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3 years ago

How many moles of methane will react to form 3.2 moles of carbon dioxide?

Chemistry

1 answer:

Hunter-Best [27]3 years ago

6 0

Answer:

3.2 moles

Explanation:

First, we'll begin by writing a balanced equation for the Combustion of methane to produce carbon dioxide. This is illustrated below:

CH4 + 2O2 —> CO2 + 2H2O

From the balanced equation above,

1 mole of methane (CH4) reacted to produced 1 mole of carbon dioxide (CO2).

Therefore, 3.2 moles of methane (CH4) will react to produce 3.2 moles of carbon dioxide (CO2).

From the illustration above, 3.2 moles of methane is needed to produce 3.2 moles of carbon dioxide.

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How do sand dunes move?<br> Use the terms leeward and windward in your explanation.

gogolik [260]

As the sand mound grows, the point of maximum sand deposition on the leeward face moves closer to the summit, causing a steepening of the leeward face relative to the windward face. The steepening and growing dune now forces wind out over the top of the dune rather than down the leeward face.

7 0

3 years ago

Consider the following properties of the atmosphere of the planet Mars at a particular measurement point on the surface, as meas

Airida [17]

Answer:

a. 581.4 Pa

b. 3.33x10⁻⁴ mol/L

c. 3.49x10⁻⁴ mol/L

d. 0.015 g/L

Explanation:

a. By the Raoult's Law, the partial pressure of a component of a gas mixture is its composition multiplied by the total pressure, so:

pA = 0.9532*6.1

pA = 5.81452 mbar

pA = 5.814x10⁻³ bar

1 bar ----- 10000 Pa

5.814x10⁻³ bar--- pA

pA = 581.4 Pa

b. Considering the mixture as an ideal gas, let's assume the volume as 1,000 L, so by the ideal gas law, the total number of moles is:

PV = nRT

Where P is the pressure (610 Pa), V is the volume (1 m³), n is the number of moles, R is the gas constant (8.314 m³.Pa/mol.K), and T is the temperature.

n = PV/RT

n = (610*1)/(8.314*210)

n = 0.3494 mol

The number of moles of CO₂ is (V = 0.9532*1 = 0.9532 m³):

n = PV/RT

n = (581.4*0.9532)/(8.314*210)

n = 0.3174 mol

cA = n/V

cA = 0.3174/953.2

cA = 3.33x10⁻⁴ mol/L

c. c = ntotal/Vtotal

c = 0.3494/1000

c = 3.49x10⁻⁴ mol/L

d. The molar masses of the gases are:

CO₂: 44 g/mol

N₂: 28 g/mol

Ar: 40 g/mol

O₂: 32 g/mol

CO: 28 g/mol

The molar mass of the mixture is:

M = 0.9532*44 + 0.027*28 + 0.016*40 + 0.0008*28 = 43.36 g/mol

The mass concentration is the molar concentration multiplied by the molar mass:

3.49x10⁻⁴ mol/L * 43.36 g/mol

0.015 g/L

8 0

3 years ago

The nearest whole number of 99.59

Anna [14]

It is 100 because a 5 and up means you round up. also the 9 makes it a 6 rounded up

7 0

3 years ago

Read 2 more answers

Find the enthalpy of neutralization of HCl and NaOH. 87 cm3 of 1.6 mol dm-3 hydrochloric acid was neutralized by 87 cm3 of 1.6 m

olga nikolaevna [1]

Explanation:

The reaction equation for the given reaction will be as follows.

$HCl + NaOH \rightarrow NaCl + H_{2}O$

Each mole of both HCl and NaOH gives one mole of water.

Also, it is given that 1 liter of NaOH and HCl solution contains 1.6 mol $dm^{-3}$ of NaOH (HCl).

It is known that 1 $cm^{3}$ = 0.001 liter. So, 87 $cm^{3}$ = 0.087 liter.

Hence, number of moles of water obtained from the given reaction are as follows.

0.087 liter × 1.6 mol = 0.1392 moles

No. of moles = $\frac{mass}{molar mass of water}$

0.1392 moles = $\frac{mass}{18 g/mol}$

mass = 2.5056 g

Now, volume of water present before the reaction is $2 \times 0.087$ liter = 0.174 liter or 0.174 Kg (as density is 1 $Kg/cm^{3}$ ) or 174 g (as 1 kg = 1000 g).