Answer: The partial pressure of
is 1.86 atm
Explanation:
Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as 
The given balanced equilibrium reaction is,

Pressure at eqm. 0.973 atm 0.548atm x atm
The expression for equilibrium constant for this reaction will be,

Now put all the given values in this expression, we get :

By solving the term 'x', we get :
x = 1.86 atm
Thus, the partial pressure of
is 1.86 atm
The answer your looking for is a)
-please give me brainliest answer
Answer:
1859.4 g of ZnCrO₄ in 10.25 moles
Explanation:
First of all, we determine the molecular formula of the compound:
Zinc → Zn²⁺ (cation)
Chromate → CrO₄⁻² (anion)
Zinc chromate → ZnCrO₄
Molar mass for the compound is:
Molar mass of Zn + Molar mass of Cr + (Molar mass of O) . 4 = 181.41 g/mol
65.41 g/mol + 52 g/mol + 16 g/mol . 4 = 181.41 g/mol
Let's apply this conversion factor: 10.25 mol . 181.41 g/mol = 1859.4 g