Question

# (b) The reaction: 4N2O + CH4 $\stackrel{}{\to }$ CO2 + 2H2O + 4N2 takes place in the gaseous state. If all volumes are measured at the same temperature and pressure, calculate the volume of dinitrogen oxide (N2O) required to give 150 cm3 of steam. (N = 14, O = 16, C = 12, H = 1)

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Solution

## According to the balanced chemical equation, four moles of di-nitrogen oxide forms two moles of steam. 1 mole of gas occupy 22.4 L or 22400 cm3 volume. Volume of two moles of steam will be 2$×$22400 cm3 Volume of 4 moles of steam will be 4 $×$ 22400 cm3 Volume of N2O required to produce (2 $×$ 22400) cm3 of steam = (4 $×$ 22400) cm3 Volume of N2O required to produce 150 cm3 of steam = $\left(\frac{150×4×22400}{2×22400}\right){\mathrm{cm}}^{3}=300{\mathrm{cm}}^{3}$

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