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Hello student.
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In this question, we are going to discuss about the calculation method of the total pressure at equilibrium.
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Here, this equation is given where a solid carbon is burnt in presence of hydrogen gas to form the methane gas.
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So previously as we discussed that we will calculate the total pressure.
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So we have to clear about one concept.
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The pressure will be only exerted by this hydrogen gas and this methane gas.
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So we know pv equals to n r t where p is the pressure, v is the volume, n is the number of moles present, r is the gas constant and t is the temperature.
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From this equation we can calculate the pressure exerted by the high, hydrogen gas that is equals to nrt by v.
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The n will be 5 .827 whole divided by 2.
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As in the question, it is mentioned that 5 .8 to 7 grams of hydrogen in present and 2 molecule is used.
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So the mole will be this.
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And r will be 0 .0821 atmosphere, liter atmosphere, and temperature is thousand.
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And the total volume is 9 .92.
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So here we will get the ph 2 as 24 .11 atm.
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This is the first step for our calculation.
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At t equals to zero, the pressure exerted by the carbon is zero, the methane gas is zero, and the hydrogen gas will be 24 .11.
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And after certain time, if we considered the pressure exerted by this methane gas is x, then the hydrogen gas will be 24 .11 minus 2 .8.
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As two molecules of hydrogen is taking part in the reaction.
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So kp will be pressure of ch4 divided by pressure of hydrogen gas.
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As two molecule is taking part, so this will be squared...