The equation for the reaction in stage 3 is shown.4N*O_{2} + 2H_{2}*O + O_{2} -> 4HNOCalculate the volume of O, gas, at room temperature and pressure ( r .t.p.) . needed to produce 1260g of HNO3. Use the following steps.11:55 AMCalculate the number of moles of HNO3.moles of HNO3 =Deduce the number of moles of O_{2} that reacted.moles of O_{2} =Calculate the volume of O2 gas that reacts at room temperature and pressure (r.t.p.).volume of O2 gas =dm³ [4]
Question
The equation for the reaction in stage 3 is shown.4N*O_{2} + 2H_{2}*O + O_{2} -> 4HNOCalculate the volume of O, gas, at room temperature and pressure ( r .t.p.) . needed to produce 1260g of HNO3. Use the following steps.11:55 AMCalculate the number of moles of HNO3.moles of HNO3 =Deduce the number of moles of O_{2} that reacted.moles of O_{2} =Calculate the volume of O2 gas that reacts at room temperature and pressure (r.t.p.).volume of O2 gas =dm³ [4]
Solution
Sure, let's solve this step by step.
Step 1: Calculate the number of moles of HNO3.
The molar mass of HNO3 is approximately 63 g/mol. So, to find the number of moles, we divide the mass by the molar mass.
moles of HNO3 = 1260 g / 63 g/mol = 20 mol
Step 2: Deduce the number of moles of O2 that reacted.
From the balanced chemical equation, we can see that 1 mole of O2 is needed to produce 4 moles of HNO3. So, to find the number of moles of O2, we divide the number of moles of HNO3 by 4.
moles of O2 = 20 mol / 4 = 5 mol
Step 3: Calculate the volume of O2 gas that reacts at room temperature and pressure (r.t.p.).
At room temperature and pressure, 1 mole of any gas occupies 24 dm³. So, to find the volume, we multiply the number of moles by 24.
volume of O2 gas = 5 mol * 24 dm³/mol = 120 dm³
So, 120 dm³ of O2 gas is needed to produce 1260 g of HNO3 at room temperature and pressure.
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