Answer: Increasing the concentration of a reactant or decreasing the concentration of the product.
Explanation: For the equilibrium of the reaction to shift to the left, we must decrease the concentration of a reactant or increase the concentration of the product. This is based on Le Chatelier's principle which describes the effect on the equilibrium of changes in concentration or pressure of a product or a reactant. Adding more products in a system would disturb the equilibrium thus it would cause to reestablish it by shifting the reaction to the left producing the reactants. This would also be the same when you decrease the number of reactants in the system.
<u>Answer:</u> The pressure of carbon dioxide gas is 11 atm
<u>Explanation:</u>
To calculate the pressure of gas, we use the equation given by ideal gas equation:
PV = nRT
where,
P = pressure of the gas = ?
V = Volume of gas = 25 L
n = number of moles of gas = 10 mole
R = Gas constant = 
T = temperature of the gas = 325 K
Putting values in above equation, we get:
Hence, the pressure of carbon dioxide gas is 11 atm
The pH of a liquid substance is calculated through the equation,
pH = -log[H3O+]
Substituting the given concentration of the hydronium ion to the equation above,
pH = -log[4.7x10^-4 M]
The value of pH is equal to 3.33. Thus, the pH of the solution is approximately 3.33.
Answer:
you divide 71.5 by 2
Explanation:
it's may look intimidating but the question is actually really simple.
