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Hi everyone.
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In this question, how many grams of phosphine can form when 26 .5 gram of phosphorus and 89 .6 liter of hydrogen gas react at stp.
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So we are given this unbalanced reaction.
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So first, we have to balance this reaction.
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So here i'm using the stochometric coefficient four in phosphine and stochometric coefficient six in hydrogen so that this reaction is balanced.
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So we have four phosphorus atom on both side and 12 hydrogen atom on both side of this reaction.
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Now in this reaction i can say 1 mole of p4 react with 6 mol of hydrogen and they can form 4 mole of phosphine.
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So let us see the data given we are given mass of a p4 that is equal to 26 .5 gram and we are given volume of hydrogen gas at stp that is standard temperature pressure condition 89 .6 liter and we have to find out the mass of phosphine produced in this rate.
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So from all concept we know one mole of a gas occupy a volume of 22 .4 liter at standard temperature and pressure condition.
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So here we are given volume and volume of hydrogen.
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So we first want to calculate the number of moles of hydrogen...