Which one has more density? Concrete Block Styrofoam

Nitrogen and hydrogen combine at a high temperature, in the presence of a catalyst, to produce ammonia. N 2 ( g ) + 3 H 2 ( g )

seraphim [82]

Answer:

0.440 moles of NH₃ are produced

Explanation:

First of all, we need to determine the limiting reactant by the stoichiometry.

Equation reaction is: N₂(g) + 3H₂(g) ⟶ 2 NH₃(g)

1 mol of nitrogen needs 3 moles of hydrogen to react

Therefore 0.220 moles of N₂ will need (0.220 . 3) / 1 = 0.660 moles of H₂

As we have 0.717 moles of H₂ and we need 0.660, the hydrogen is the excess reagent, therefore, the N₂ is the limiting reactant

3 moles of H₂ need 1 mol of N₂ to react

Then, 0.717 moles of H₂ will react with (0.717 . 1) / 3 = 0.239 moles of N₂

We do not have enough N₂

After complete reaction → ratio is 1:2

1 mol of N₂ reacts to produce 2 moles of ammonia

Therefore 0.220 moles of N₂ will produce (0.220 . 2) / 1 = 0.440 moles of NH₃

6 0

4 years ago

The repeating subunits that are responsible for the chance of a crystal are know as

Naddik [55]

Unit cells.
They are the smallest group of atoms that take form of a crystal and can repeat in 3 dimensions.

7 0

3 years ago

4. what reaction fuels the burning of the sun? A.fission B.fusion C.combustion D.transmutation

Lostsunrise [7]

Answer:

A

Explanation:

7 0

3 years ago

Read 2 more answers

Nickel and carbon monoxide react to form nickel carbonyl, like this: (s)(g)(g) At a certain temperature, a chemist finds that a

horsena [70]

The question is incomplete, here is the complete question:

Nickel and carbon monoxide react to form nickel carbonyl, like this:

$Ni(s)+4CO(g)\rightarrow Ni(CO)_4(g)$

At a certain temperature, a chemist finds that a 2.6 L reaction vessel containing a mixture of nickel, carbon monoxide, and nickel carbonyl at equilibrium has the following composition:

Compound Amount

Ni 12.7 g

CO 1.98 g

$Ni(CO)_4$ 0.597 g

Calculate the value of the equilibrium constant.

Answer: The value of equilibrium constant for the reaction is 2448.1

Explanation:

We are given:

Mass of nickel = 12.7 g

Mass of CO = 1.98 g

Mass of $Ni(CO)_4$ = 0.597 g

Volume of container = 2.6 L

To calculate the number of moles for given molarity, we use the equation:

$\text{Molarity of the solution}=\frac{\text{Given mass of solute}}{\text{Molar mass of solute}\times \text{Volume of solution (in L)}}$

$\text{Equilibrium concentration of nickel}=\frac{12.7}{58.7\times 2.6}=0.083M$

$\text{Equilibrium concentration of CO}=\frac{1.98}{28\times 2.6}=0.0272M$

$\text{Equilibrium concentration of }Ni(CO)_4=\frac{0.597}{170.73\times 2.6}=0.00134M$

For the given chemical reaction:

$Ni(s)+4CO(g)\rightarrow Ni(CO)_4(g)$

The expression of equilibrium constant for the reaction:

$K_{eq}=\frac{[Ni(CO)_4]}{[CO]^4}$

Concentrations of pure solids and pure liquids are taken as 1 in equilibrium constant expression.

Putting values in above expression, we get:

$K_{eq}=\frac{0.00134}{(0.0272)^4}\\\\K_{eq}=2448.1$

Hence, the value of equilibrium constant for the reaction is 2448.1

4 0

4 years ago

When aqueous solutions of Li3PO4 and MgSO4 are mixed, Mg3(PO4)2 is a precipitate

Lesechka [4]

Answer:

Li2SO4

Explanation:

Balance the reaction of Li3PO4 + MgSO4 = Li2SO4 + Mg3(PO4)2 using this chemical equation balancer!

8 0

3 years ago