MassWhat is the percent composition by mass of
nitrogen in the compound N,H, (gram-formula
32 g/mol)?
(1) 13%
(3) 88%
(2) 44%
(4) 93%

The mass of hydrogen gas obtained is 0.068 g of hydrogen gas.

The equation of the reaction is;

Ca(s) +2H2O(l) →Ca(OH)2(aq) + H2(g)

We have to obtain the number of moles of hydrogen gas produced using the information in the question.

P =  988mmHg - 17.54 mmHg = 1.28 atm

V = 641 mL or 0.641 L

T = 20 + 273 = 293 K

n = ?

R = 0.082 atmLK-1mol-1

From;

PV = nRT

n = PV/RT

n = 1.28 atm × 0.641 L/ 0.082 atmLK-1mol-1 × 293 K

n = 0.82/24.026

n = 0.034 moles

Mass of hydrogen =  0.034 moles × 2 g/mol = 0.068 g of hydrogen gas

Learn more: brainly.com/question/1445383

Answer:

There is 0.0677 grams of H2 gas obtained

Explanation:

Step 1: Data given

The total pressure (988 mmHg) is the sum of the pressure of the collected hydrogen + the vapor pressure of water (17.54 mmHg).  

ptotal = p(H2)+ p(H2O)

p(H2) = ptotal - pH2O = 988 mmHg - 17.54 mmHg = 970.46 mmHg

Step 2: Calculate moles of H2 gas

Use the ideal gas law to calculate the moles of H2 gas

PV = nRT

n = PV / RT

 ⇒ with p = pressure of H2 in atm = 970.46 mmHg * (1 atm /760 mmHg) = 1.277 atm

⇒ V = volume of H2 in L = 641 mL x (1 L / 1000 mL) = 0.641 L

⇒ n = the number of moles of H2 = TO BE DETERMINED

⇒ R = the gas constant = 0.08206 L*atm/K*mol

⇒ T = the temperature = 20.0 °C = 293.15 Kelvin

n = (1.277)(0.641) / (0.08206)(298.15) = 0.0335 moles H2

Step 3: Calculate mass of H2

Mass of H2 = moles H2 ¨molar H2

0.0335 moles H2 * 2.02 g/mol H2  = 0.0677g H2

There is 0.0677 grams of H2 gas obtained

Answer:

1. Proton = electron if the element is not in an ionic state

proton = atomic number

Answer:

Ba(OH)2 (aq) + H2SO4(aq) → BaSO4(s) + 2 H2O(l)

That's the right one.

Explanation:

You should see that this equation is balanced, not as

Ba(OH)2 (aq) + H2SO4(aq) → BaSO4(s) + H2O(l)

(on reactive we have 4 H, on products, we have only 2)

Ba(OH)2 (aq) + H2SO4(aq) → H2Ba(s) + SO4(OH)2(l)

(this is impossible, it's a nonsense)

BaSO4(s) + 2 H2O(l) → Ba(OH)2 (aq) + H2SO4(aq)

(it is the same with the right one but is the other way around. The statement says, reaction of Ba(OH)2 with H2SO4, not BaSO4 with water. Also, it is not a chemical balance.

Answer:

Its arrangement.

Explanation:

Hello,

In this case, we rewrite the chemical reaction as:

Now, a more organized dimensional analysis is shown below to determine the very same required value:

Without giving the numerical answer, one sees that the student's dimensional analysis is wrongly written as long as the 3 moles of must be dividing rather than multiplying as it is the relationship factor used to relate it with the based on the reaction stoichiometry. Moreover, the 6.7moles of must be multiplying as it is the starting value.

Best regards.

Answer:

The error is in the rule of three.

3 mol of Ba(OH)2 ___ comes from ____ 1 mol Ba3N2

6.7 mol of Ba(OH)2 ___ comes from ___ (6.7 .1) / 3

Explanation:

Ba3N2 + 6H2O → 3Ba(OH)2 + 2NH3

3 mol of Ba(OH)2 x 1 mol of Ba3N2 / 6.7 mol of Ba(OH)2

- The rule of three is wrong.

- The chemical equation is ballanced.

- The question is not clear about which is the limiting reactant. May be we don't have enough water, so that's the limiting and Ba3N2 is in excess. So have to work with H2O.

Answer:

Reactants

Explanation: