If 1.0 mole of CH4 and 2.0 moles of Cl2 are used in the reaction CH4 + 4Cl2 => CCl4 + 4HCl then which of these statements is
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Answer:- 38.2 g.
Solution:- The equation used for solving this type of calorimetry problems is:
where, q is the heat energy, m is mass, c is specific heat and delta T is the change in temperature.
Water temperature is increasing from 14.5 degree C to 50.0 degree C.
= 35.5 degree C
q is given as 5680 J and specific heat value is .
The equation could be rearranged for m as:
Let's plug in the values in it:
m = 38.2 g
So, the mass of water in the kettle is 38.2 g.
Answer:
pCH₄ = 105.1 - 0.42 = 104.68 torr
pI₂ = 7.96 -0.42 = 7.54 torr
pCH₃I = 0.42 torr
pHI = 0.42 torr
Explanation:
Kp is the equilibrium constant for the partial pressure of the gases in the reaction, and it is calculated for a general equation:
aA(g) + bB(g) ⇄ cC(g) + dD(g)
, where p is the partial pressure in the equilibrium. By the reaction given:
CH₄(g) + I₂(g) ⇄ CH₃I(g) + HI(g)
105.1 torr 7.96 torr 0 0 <em> initial partial pressure</em>
-x -x +x +x <em> react</em>
105.1-x 7.96-x x x <em>equilibrium</em>
Then:
x² = 0.1891 - 0.0255x -2.26x10⁻⁴x²
0.9997x² + 0.0255x - 0.1891 = 0
Using Bhaskara's rule:
Δ = (0.0255)² - 4x(0.9997)x(-0.1891)
Δ = 0.7568
Using only the positive term, x = 0.42 torr.
So,
pCH₄ = 105.1 - 0.42 = 104.68 torr
pI₂ = 7.96 -0.42 = 7.54 torr
pCH₃I = 0.42 torr
pHI = 0.42 torr