All categories

3 years ago

What is the correct formula for the compound formed between magnesium and the phosphate ion?

Chemistry

1 answer:

tino4ka555 [31]3 years ago

8 0

Answer:

The formula would be Mg3P2 . This would be an ionic compound.

Explanation:

You might be interested in

A rigid, closed vessel of volume V =648 liters maintained at constant temperature T=365 K is loaded with 112 mol of n-hexane, 15

Marrrta [24]

Answer:

P = 2.92 atm

Explanation:

With the three assumptions in mind, the system consists of:

A liquid phase containing n-hexane and n-heptane, and

A gaseous phase containing n-hexane vapor, n-heptane vapor, and nitrogen gas.

First we use PV=nRT to calculate the moles of n-hexane and n-heptane in the gaseous phase:

n-hexane:

P = 0.199 MPa ⇒ 0.199 * 1.869 = 1.964 atm

1.964 atm * 648 L = n * 0.082 atm·L·mol⁻¹·K⁻¹ * 365 K

n = 42.52 moles

n-heptane:

P = 0.083 MPa ⇒ 0.083 * 1.869 = 0.155 atm

0.155 atm * 648 L = n * 0.082 atm·L·mol⁻¹·K⁻¹ * 365 K

n = 3.358 moles

So the gaseous phase consists of 42.52 moles of n-hexane, 3.358 moles of n-heptane, and 14 mol of nitrogen.

For the liquid phase, we calculate the remaining moles of n-hexane and n-heptane. Then we convert to liters, using their molar volumes:

n-hexane:

n = 112 mol - 42.52 mol = 69.48 mol

69.48 mol * 0.146 L/mol = 10.14 L

n-heptane:

n = 155 mol - 3.358 mol = 151.642 mol

151.642 mol * 0.162 L/mol = 24.57 L

So the liquid phase occupies (10.14+24.57) = 34.71 L, and contains 69.48 mol of n-hexane and 151.64 mol of n-heptane.

Finally, to calculate the pressure in the vessel, we use PV=nRT:

P = ?

V = 648 - 34.71 = 613.29 L

n = 42.52 mol hexane + 3.35 mol heptane + 14 mol nitrogen = 59.87 mol

T = 365 K

P * 613.29 L = 59.87 mol * 0.082 atm·L·mol⁻¹·K⁻¹ * 365 K

P = 2.92 atm

6 0

3 years ago

how many atoms of phosphorous are in 4.90 mol of copper(ii) phosphate? the formula for copper(ii) phosphate is Cu3(PO4)2.

Karolina [17]

Answer:

$\boxed{5.90 \times 10^{24}}$

Explanation:

Step 1. Calculate the formula units of Cu₃(PO₄)₂

$\text{4.90 mol Cu$_{3}$(PO$_{4}$)$_{2}$} \times \dfrac{6.022 \times 10^{23} \text{ formula units}}{\text{1 mol Cu$_{3}$(PO$_{4}$)$_{2}$}}\\\\=\text{2.951 $\times$ 10$^{24}$ formula units Cu$_{3}$(PO$_{4}$)$_{2}$}$

Step 2. Calculate the atoms of P

$\text{Atoms of P}\\\\=\text{2.951 $\times$ 10$^{24}$ formula units Cu$_{3}$(PO$_{4}$)$_{2}$} \times \dfrac{ \text{2 atoms P}}{\text{1 formula unit Cu$_{3}$(PO$_{4}$)$_{2}$}}\\\\= \boxed{5.90 \times 10^{24} \text{ atoms P}}$

8 0

3 years ago

Consider the following chemical equation: NH4NO3(s)⟶NH+4(aq)+NO−3(aq) What is the standard change in free energy in kJmol at 298

Galina-37 [17]

Answer:

$\Delta _rG=-4.3\frac{kJ}{mol}$

Explanation:

Hello,

In this case, for the given dissociation reaction, we can compute the enthalpy of reaction considering the enthalpy of formation of each involved species (products minus reactants):

$\Delta _rH=\Delta _fH_{NH^{4+}}+\Delta _fH_{NO_3^-}-\Delta _fH_{NH_4NO_3}\\\\\Delta _rH=-132.5+(-205.0)-(-365.6)=28.1kJ/mol$

Next, the entropy of reaction considering the standard entropy for each involved species (products minus reactants):

$\Delta _rS=S_{NH^{4+}}+S_{NO_3^-}-S_{NH_4NO_3}\\\\\Delta _rS=113.4+146.4-151.1=108.7J/mol*K$

Next, since the Gibbs free energy of reaction is computed in terms of both the enthalpy and entropy of reaction at the given temperature (298.15 K), we finally obtain (two significant figures):

$\Delta _rG=\Delta _rH-T\Delta _rS\\\\\Delta _rG=28.1kJ/mol-(298.15 K)(108.7\frac{J}{mol*K}*\frac{1kJ}{1000J} )\\\\\Delta _rG=-4.3\frac{kJ}{mol}$

Best regards.

6 0

3 years ago

The following data was collected for the formation of ammonia (NH3) based on the following overall reaction: N2 + 3H2 = 2NH3 N2

notsponge [240]

Answer : The unit for the rate constant in the rate law for the formation of ammonia is, $M^{-2}min^{-1}$

Explanation :

Rate law is defined as the expression which expresses the rate of the reaction in terms of molar concentration of the reactants with each term raised to the power their stoichiometric coefficient of that reactant in the balanced chemical equation.

For the given chemical equation:

$N_2+3H_2\rightarrow 2NH_3$