How much heat is absorbed during the reaction of 48.0 grams of O2 with excess nitrogen in the following reaction if ΔH = 68 kJ/mol N2?"

Answers

Answer 1

Answer: Chemistry is hard………

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SE DESEA OBTENER UNA SOLUCION 0.3 MOLARIDAD DE HIDROXIDO DE POTASIO DISOLVIENDO 60 GRAMOS DE HIDROXIDO -¿QUE VOLUMEN DE SOLUCION SE OBTENDRA QUIMICA

Answers

Answer:

3.56L will be the obtained volume

Explanation:

0.3 M → Molarity

These are the moles of solute (for this case, the solute is KOH) that are contianed in 1L of solution

We dissolved 60 g of solute, so let's determine the moles:

60 g . 1 mol/ 56.1 g = 1.07 moles

Molarity(mol/L) = Mol / Volume(L)

Let's replace data: 0.3M = 1.07 mol / Volume(L)

0.3 mol/L = 1.07 mol / volume

Volume = 1.07 mol / 0.3mol/L = 3.56 L

43. Which temperature change would cause a sample of an ideal gas to double in volume while the pressure is held constant?(1) from 400.K to 200.K(2) from 200.K to 400.K
(3) from 400.oC to 200.oC
(4) from 200.oC to 400.oC

Answers

This question may be answered by looking at the equation for ideal gases. The ideal gas equation is pV = nRT. Which implies that If pressure is constant (n is constant if the amount of gas is not changed and R is the Universal Constant of Gases), then V / T is constant. Then if V is doubled T is also doubled. Then the answer is the option (2) from 200K to 400K..

H2SO3
Spell out the full name of the compound.

Answers

sulfurous acid or sulphurous acid

The full name of this compound/ acid is:
Sulfurous acid or Sulphorous acid

... Remember SO3 is a ployatomic ion ending in -ite..
.... I hope it helps!

Calculate the number of atoms in 4g of bromine molecule.(Br).(avogadro 's constant =6.02 x 10²³ mol-¹; Br=80)

Answers

Answer:

$\n N=n * N_(A)$

We do not have $n$ - the amount of substance.

$n=(m)/(M)\n$

The molecular weight ( $M$ ) of Bromine is 80.

$n=(4)/(80) = 0.05 \text{ mol}$

$N = 0.05 * 6.02 * 10^(23) = 0.301 * 10^(23)$

Whats another name for a group of elements ?

Answers

family. IDK why they call it but i remembered

Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride: S(g) + 3F2(g) ->SF6(g) If 50 g S is allowed to react as completely as possible with 105.0g F2(g), what mass of the excess reactant is left.

Answers

Answer: The mass of excess reagent left is 20.48 g

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

For sulfur:

Given mass of sulfur = 50 g

Molar mass of sulfur = 32 g/mol

Putting values in equation 1, we get:

$\text{Moles of sulfur}=(50g)/(32g/mol)=1.56mol$

For fluorine gas:

Given mass of fluorine gas = 105 g

Molar mass of fluorine gas = 37.99 g/mol

Putting values in equation 1, we get:

$\text{Moles of fluorine gas}=(105g)/(37.99g/mol)=2.76mol$

The chemical equation for the reaction of sulfur and fluorine gas follows:

$S(g)+3F_2(g)\rightarrow SF_6(g)$

By Stoichiometry of the reaction:

3 moles of fluorine gas reacts with 1 mole of sulfur

So, 2.76 moles of fluorine gas will react with = $(1)/(3)* 2.76=0.92mol$ of sulfur

As, given amount of sulfur is more than the required amount. So, it is considered as an excess reagent.

Thus, fluorine gas is considered as a limiting reagent because it limits the formation of product.

Moles of excess reagent (sulfur) left = 1.56 - 0.92 = 0.64 moles

Now, calculating the mass of sulfur from equation 1, we get:

Molar mass of sulfur = 32 g/mol

Moles of sulfur = 0.64 moles

Putting values in equation 1, we get:

$0.64mol=\frac{\text{Mass of sulfur}}{32g/mol}\n\n\text{Mass of sulfur}=20.48g$

Hence, the mass of excess reagent left is 20.48 g

The mole number of 50 g S is 1.563 mol. 105.0 g F2 is 2.763 mol. The ratio of S and F2 is 1:3. So the excess one is S. And mass left is 0.642*32=20.52 g.

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