CHEMISTRY COLLEGE

Be sure to answer all parts. Industrially, hydrogen gas can be prepared by combining propane gas (c3h8) with steam at about 400°c. The products are carbon monoxide (co) and hydrogen gas (h2). (a) write a balanced equation for the reaction. Include phase abbreviations. (b) how many kilograms of h2 can be obtained from 8.31 × 103 kg of propane

Answers

Answer 1

Answer:

Balanced chemical reaction:

C₃H₈(g) + 3H₂O(g) → 3CO(g) + 7H₂(g).

M(C₃H₈) = 44.1 g/mol; molar mass of propane.

M(H₂) = 2 g/mol; molar mass of hydrogen.

From balanced chemical reaction: n(C₃H₈) : n(H₂) = 1 : 7.

7m(C₃H₈) : M(C₃H₈) = m(H₂) : M(H₂).

7·8310 kg : 44.1 g/mol = m(H₂) : 2 g/mol.

m(H₂) = 2638.09 kg; mass of hydrogen.

Answer 2

Answer:

Answer: a) $C_3H_8(g)+3H_2O(g)\rightarrow 3CO(g)+7H_2(g)$

b) $2.64* 10^3kg$

Explanation:

a) According to the law of conservation of mass, mass can neither be created nor be destroyed. Thus the mass of products has to be equal to the mass of reactants. The number of atoms of each element has to be same on reactant and product side. Thus chemical equations are balanced.

$C_3H_8(g)+3H_2O(g)\rightarrow 3CO(g)+7H_2(g)$

b) $\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

$\text{Number of moles of propane}=(8.31* 10^6g)/(44.1g/mol)=0.188* 10^6moles$

$C_3H_8(g)+3H_2O(g)\rightarrow 3CO(g)+7H_2(g)$

According to stoichiometry:

1 mole of $C_3H_8$ gives 7 moles of $H_2$

Thus $0.188* 10^6moles$ moles of $C_3H_8$ will give = $(7)/(1)* 0.188* 10^6=1.32* 10^6moles$ of $H_2$

Mass of $H_2=moles* {\text {molar Mass}}=1.32* 10^6moles* 2g/mol=2.64* 10^6g=2.64* 10^3kg$

Thus $2.64* 10^3kg$ of $H_2$ can be obtained from $8.31* 10^3$ kg of propane

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A gas mixture with a total pressure of 770 mmHg contains each of the following gases at the indicated partial pressures: 128 mmHg CO2, 232 mmHg Ar, and 183 mmHg O2. The mixture also contains helium gas. What is the partial pressure of the helium gas?

Answers

The partial pressure of Helium gas can be calculated by applying Daltons law of partial pressure and that comes out to be 227 mmHg.

What is Dalton's law of partial pressure?

Dalton's law of partial pressure helps in calculating the total pressure exerted by all the gases that are present in a mixture that is equal to the sum of partial pressure of all individual gases.

Partial pressure is the pressure that is exerted by one gas in a mixture of gases on the walls of the container. This law is applicable to only mixture of gases that are ideal gases. Ideal gases are the one which do not have any forces of attraction or repulsion between the particles of thee gas.

In our question

$p_(total) =p_{CO_(2) }+p_(Ar)+p_{O_(2) } +p_{{He} }$

$p_{{He} } =p_(total)-[p_{CO_(2) }+p_(Ar)+p_{O_(2) } ]$

substituting all given values

$p_{{He} } =770-(128+232+183)$

=227mmHg

Thus the partial pressure of Helium gas is 227mmHg

To learn more about Dalton's law of partial pressure, here:

brainly.com/question/14119417

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Answer:

227 mmHg

Explanation:

Ptotal= PCO2 +PAr+PO2+PHe

PHe= Ptotal-PCO2 -PAr-PO2

PHe= (770 mmHg)-(128 mmHg)-(232 mmHg)-(183 mmHg)

PHe=227 mmHg

1. The common name for the compound CH3-CH2-O-CH3 is

Answers

Answer:

propane

Explanation:

please mark me as brainliest

Answer:

Methoxyethane also known as ethyl methyl ether

The osmotic pressure, π, of a solution of glucose is 132 atm . find the molarity of the solution at 298 k.

Answers

The formula for osmotic pressure is:

$\Pi = iMRT$

where $\Pi$ is osmotic pressure, $i$ is van't Hoff's factor, $M$ molarity, $R$ is Ideal gas constant, and T is Temperature.

$\Pi$ = 132 atm

The van't Hoff's factor for glucose, $i$ = 1

$R = 0.08206 Latmmol^(-1)K^(-1)$

$T = 298 K$

Substituting the values in the above equation we get,

$132 atm = 1* M* 0.08206 Latmmol^(-1)K^(-1)* 298$

$M = (132 atm)/(1* 0.08206 Latmmol^(-1)K^(-1)* 298) = 5.4797 molL^(-1) \simeq 5.48 molL^(-1)$

So, the molarity of the solution is $5.48 molL^(-1)$ .

when the pressure that a gas exerts on a sealed container changes from 3.74 atm to ____ atm, the temperature changes from 394 K to 789 K

Answers

Gay-Lussacs law gives the relationship between pressure and temperature of a gas.
It states that pressure of gas is directly proportional to the temperature at constant volume.
P/T = k
Where k - constant
P1/T1 = P2/T2
Where parameters for the first instance are on the left side and parameters for the second instance on the right side of the equation.
3.74 atm /394 K = P/789 K
P = 7.49 atm

Answer:

7.49 atm

Explanation:

What product would you expect from a nucleophilic substitution reaction of (S)-2-bromohexane with acetate ion, CH3CO22? Assume that inversion of configuration occurs, and show the stereochemistry of both the reactant and product.

Answers

Answer:

(R) - hexyl acetate

Explanation:

Hello,

This reacción is a nucleophilic substitution SN2.

The configuration (s), means that the groups around the chiral carbon are organized appose to the clock hands movement. But when the reaction happens, these configurations become an (r) configuration, it means the groups around the chiral carbon organize according to the clock hands movement.

Generally, these reactions are related to nucleophilic species, an example is the ion acetate, a conjugated acid which is a weak nucleophilic, for this reason, the transition state is more energetic, it means, less stable than if the reaction occurs with a strong nucleophilic.

Look the image to compare the two configurations of the reactant and product.

Note: Please show all work and calculation setups to get full credit. T. he following may be used on this assignment: specific heat of (water=4.184 J/g oC; ice=2.03 J/g oC; steam=1.99 184 J/g oC); heat of fusion of water=80. cal/g; heat of vaporization=540 cal/g; 1cal=4.184J.Calculate the energy required (in J) to convert 25 g of ice at -15 oC to water at 75 oC.