If 0.332 mol of zinc reacts with excess lead(IV) sulfate, how many grams of zinc sulfate will be produced in the reaction?

53.6 g

Explanation:

Step 1: Write the balanced equation

2 Zn + Pb(SO₄)₂ ⇒ 2 ZnSO₄ + Pb

Step 2: Calculate the moles of ZnSO₄ produced from 0.332 moles of Zn

The molar ratio of Zn to ZnSO₄ is 2:2. The moles of ZnSO₄ produced are 2/2 × 0.0332 mol = 0.0332 mol.

Step 3: Calculate the mass corresponding to 0.332 moles of ZnSO₄

The molar mass of ZnSO₄ is 161.44 g/mol.

0.332 mol × 161.44 g/mol = 53.6 g

these nuts

a: 45.9 meters

b: 4.29 seconds

step-by-step explanation:

a: h(t)=1/2(-9.8)(3)^2+0(3)+90

h(t)=-4.9(3)^2+90

h(t)=-44.1+90

h(t)=45.9 meters

b: 0=1/2(-9.8)(t^2)+0t+90

0=-4.9t^2+90

-90=-4.9t^2

18.37=t^2

t=4.29 seconds

in the second question, the numbers aren't exact, but they're a close approximation.