Chemistry, 12.11.2019 04:31 ChloeLiz7111

Consider the chemical reaction:
2h2o(l)→2h2(g)+o2(g)
how many moles of h2o are required to form 1.6 l of o2 at a temperature of 324 k and a pressure of 0.984 atm ?
express your answer using two significant figures.

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The number of moles of H2O required to form 1.6 L of O2 at a temperature of 324 K and a pressure of 0.984atm is 0.118moles

To calculate the number of moles of oxygen involved in the reaction can be calculated using the following expression:

PV = nRT

Where;

P = pressure (atm)V = volume (L)n = number of moles (mol)R = gas law constant (0.0821 Latm/molK)T = temperature (K)n = (0.984 × 1.6) ÷ (0.0821 × 324)n = 1.5744 ÷ 26.6n = 0.059mol of O2. According to this reaction; 2H2O(l) → 2H2(g) + O2(g)2 moles of H2O produce 1 mole of O20.059 moles of O2 will be produced when 0.059 × 2 = 0.118moles of H2O. Therefore, the number of moles of H2O required to form 1.6 L of O2 at a temperature of 324K and a pressure of 0.984atm is 0.118moles.

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Answer from: kharmaculpepper

The answer to your question is: 0.118 moles of water

Explanation:

Data

moles of water = ?

Vol of O2= 1.6

Temp = 324°K

Pressure = 0.984 atm

R = 0.082 atm l / mol°K

Process

1.- Calculate the moles of O₂ using the ideal gas formula.

PV = nRT

$n = \frac{PV}{RT}$

$n = \frac{(1.6)(0.984)}{(0.082)(324)}$

$n = \frac{1.5744}{26.568}$

n = 0.059 moles of oxygen

2.- Find the moles of water

2 moles of water ------------------ 1 mol of oxygen

x ------------------ 0.059 moles

x = (0.059 x 2) / 1

x = 0.118 moles of water

Answer from: Quest

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Answer from: Quest

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Consider the chemical reaction:
2h2o(l)→2h2(g)+o2(g)
how many moles of h2o are required...

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