The concentration equilibrium constant is calculated as:
Kc = [CO][H2]^2 / [CH3OH] = (0.44 M)(2.7 M)^2 / (0.20 M) = 16.038 M^2
The degree of the reaction is the sum of the product coefficients minus that of the reactants: n = 1 (CO) + 2 (H2) - 1 (CH3OH) = 2
Then the pressure equilibrium constant is calculated as:
Kp = Kc*(RT)^(n) = (16.038 M^2)*[(0.08206 atm/M-K)(673.15 K)]^(2) = 48,936.95 atm^2
Remember to use absolute temperature of 400+273.15 K, not the 400 C itself.
Answer:
3.2 x 10²¹molecules
Explanation:
Given parameters:
Volume of nitrogen gas = 120cm³
Unknown:
Mass of nitrogen gas = ?
Number of molecules = ?
Solution:
To solve this problem, note that;
1 mole of gas occupies a volume of 22.4L at STP
Now;
convert 120cm³ to L ;
1000cm³ = 1L
120cm³ gives 0.12L
Since;
22.4L of gas has 1 mole at STP
0.12L of gas will have 
= 0.0054mole at STP
So;
Mass of N₂ = number of moles x molar mass
Molar mass of N₂ = 2(14) = 28g/mol
Mass of N₂ = 0.0054 x 28 = 0.15g
Now;
1 mole of a gas will have 6.02 x 10²³ molecules
0.0054 mole of N₂ will contain 0.0054 x 6.02 x 10²³ =
3.2 x 10²¹molecules
Answer:
3.97 M
Explanation:
Given data:
Initial volume V₁ = 318 mL
Initial molarity M₁ = 5.75 M
New volume V₂= 461 mL
New concentration M₂= ?
Solution:
New volume V₂= 143 mL+ 318 mL
New volume V₂= 461 mL
Formula:
M₁V₁ = M₂V₂
M₂ = M₁V₁ / V₂
M₂ = 5.75 M × 318 mL / 461 mL
M₂ = 1828.5 M. mL/ 461 mL
M₂ = 3.97 M
Nothing happens because a physical change only changes the appearance of the substance, whereas a chemical change transforms the substance into something completely different.
i.e. (chemical change) wood + fire = ash
(physical change) wood + axe = smaller pieces of wood
x(0.5)(320)=(1.2)(48)(325)
160x=18720
x=18720/160
x=117
3 significant figures
