Question

What mass of natural gas ($CH_4$) must burn to emit 275 kJ of heat?\\ $CH_4(g) + 2O_2(g) \rightarrow CO_2(g) + 2H_2O(g)$\\ $\Delta_r H^\circ = -802.3 \text{ kJ mol}^{-1}$

          What mass of natural gas ($CH_4$) must burn to emit 275 kJ of heat?\\
$CH_4(g) + 2O_2(g) \rightarrow CO_2(g) + 2H_2O(g)$\\
$\Delta_r H^\circ = -802.3 \text{ kJ mol}^{-1}$

What mass of natural gas (CH4) must burn to emit 275 kJ of heat?

CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)

H^∘ = -802.3 kJ mol^-1

Added by Brandon G.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Sima Sarker

08/14/2023

Step 1

We can use the equation ΔrH° = -802.3 kJ/mol to calculate the moles of CH4 needed. ΔrH° = -802.3 kJ/mol Heat emitted = 275 kJ Moles of CH4 = Heat emitted / ΔrH° Moles of CH4 = 275 kJ / -802.3 kJ/mol Moles of CH4 ≈ -0.343 mol Show more…

Show all steps

Thanks for your feedback!

What mass of natural gas (CH_(4)) must burn to emit 275kJ of heat? CH_(4)(g)+2O_(2)(g)->CO_(2)(g)+2H_(2)O(g) Delta _(r)Hdeg =-802.3kJmol^(-1) m= What mass of natural gas (CH4) must burn to emit 275 kJ of heat? CH4(g) + 2O2(g)->CO2(g) + 2H2O(g) rH=-802.3 kJ mol-1 V AE ? m = g Submit Request Answer