Answer:
a) 0.115 g
Explanation:
The balanced reaction is:
CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O(g)
To heat 55g of water, the energy in form of heat necessary can be calculated by:
Q = mcΔT
where Q is the heat, m is the mass, c is the specific heat (for water, c = 4.18 J/gºC), and ΔT is the variation of the temperature, which is 25ºC, so:
Q = 55x4.18x25
Q = 5747.5 J = 5.7475 kJ
So, for the reaction, 1 mol of CH₄ releases 802.3 kJ, so to release 5.7475 kJ will be necessary:
1 mol ---------------- 802.3 kJ
x ---------------- 5.7475 kJ
By a simple direct three rule:
802.3x = 5.7475
x = 7.164x10⁻³mol
The molar mass of CH₄ is : 12 (of C) + 4x1 (of H) = 16 g/mol
The mass is equal to the number of moles multiplied by molar mass, the:
m = 7.164x10⁻³x16
m = 0.115 g
The minimum mass of [tex]CH_4[/tex] is required to heat 55 g of water by 25 °C is 0.115 g.
Carbon dioxide is a gas that is made up of carbon and oxygen. This gas is used by plants to make their food.
The equation is given,
[tex]\rm CH_4(g) + 2O_2(g) \rightarrow CO_2(g) + 2H_2O(g)[/tex]
To calculate the specific heat
Q = mcΔT
where, Q is the heat
m is the mass
c is the specific heat (for water, c = 4.18 J/gºC).
ΔT is the variation of the temperature, that is 25ºC,
[tex]Q = 55\times 4.18\times 25[/tex]
Q = 5747.5 J = 5.7475 kJ
1 mole of methane produce 802.3 kJ, then to release 5.7475 kJ
By simple direct three rule:
[tex]802.3x = 5.7475\\\\x = 7.164\times10^-^3mol[/tex]
The molar mass of CH₄ is : 12 (of C) + 4x1 (of H) = 16 g/mol
Now, Calculate the mass
[tex]m = 7.164\times 10^-^3\times 16= 0.115 g[/tex]
Thus, the minimum mass of CH4 is required to heat 55 g of water by 25 °C is 0.115 g.
Learn more about methane, here:
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