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melamori03 [73]
1 year ago
8

What volume of carbon dioxide, at 1 atm pressure and 112°C, will be produced when 80.0 grams of methane is burned?

Chemistry
1 answer:
Vadim26 [7]1 year ago
6 0

Answer:

158 L.

Explanation:

What is given?

Pressure (P) = 1 atm.

Temperature (T) = 112 °C + 273 = 385 K.

Mass of methane CH4 (g) = 80.0 g.

Molar mass of methane CH4 = 16 g/mol.

R constant = 0.0821 L*atm/mol*K.

What do we need? Volume (V).

Step-by-step solution:

To solve this problem, we have to use ideal gas law: the ideal gas law is a single equation which relates the pressure, volume, temperature, and number of moles of an ideal gas. The formula is:

PV=nRT.

Where P is pressure, V is volume, n is the number of moles, R is the constant and T is temperature.

So, let's find the number of moles that are in 80.0 g of methane using its molar mass. This conversion is:

80.0g\text{ CH}_4\cdot\frac{1\text{ mol CH}_4}{16\text{ g CH}_4}=5\text{ moles CH}_4.

So, in this case, n=5.

Now, let's solve for 'V' and replace the given values in the ideal gas law equation:

V=\frac{nRT}{P}=\frac{5\text{ moles }\cdot0.0821\frac{L\cdot atm}{mol\cdot K}\cdot385K}{1\text{ atm}}=158.04\text{ L}\approx158\text{ L.}

The volume would be 158 L.

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Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of Al(C2H3O2)3 and LiNO3 are mixed. Giv
RSB [31]

Answer: No reaction occurs

Explanation:.

Spectator ions are defined as the ions which does not get involved in a chemical equation or they are ions which are found on both the sides of the chemical reaction present in ionic form.

The given chemical equation is:

Al(C_2H_3O_2)_3(aq)+3LiNO_3(aq)\rightarrow Al(NO_3)_3(aq)+3LiC_2H_3O_2(s)

The complete ionic equation is;

Al^{3+}(aq)+3C_2H_3O_2^-(aq)+3Li^+(aq)+3NO_3^-(aq)\rightarrow Al^{3+}(aq)+3NO_3^-(aq)+3Li^+(aq)+3C_2H_3O_2^-(aq)

The ions which are present on both the sides of the equation are are not involved in net ionic equation.

Hence, there is no net reaction.

5 0
3 years ago
A first order reaction has a rate constant of 0.543 at 25 c and 6.47 at 47
alukav5142 [94]

The activation energy Ea can be related to rate constant (k) at temperature (T) through the equation:

ln(k2/k1) = Ea/R[1/T1 - 1/T2]

where :

k1 is the rate constant at temperature T1

k2 is the rate constant at temperature T2

R = gas constant = 8.314 J/K-mol

Given data:

k1 = 0.543 s-1; T1 = 25 C = 25+273 = 298 K

k2 = 6.47 s-1; T = 47 C = 47+273 = 320 K

ln(6.47/0.543) = Ea/8.314 [1/298 - 1/320]

2.478 = 2.774 *10^-5 Ea

Ea = 0.8934*10^5 J = 89.3 kJ

5 0
3 years ago
A container is at a pressure of 3 atm and a temperature of 280K. What is the new temperature when the pressure is reduced to 1.5
GenaCL600 [577]

Answer:

140 K

Explanation:

Step 1: Given data

  • Initial pressure of the gas (P₁): 3 atm
  • Initial temperature of the gas (T₁): 280 K
  • Final pressure of the gas (P₂): 1.5 atm
  • Final temperature of the gas (T₂): ?

Step 2: Calculate the final temperature of the gas

We have a gas whose pressure is reduced. If we assume an ideal behavior, we can calculate the final temperature of the gas using Gay-Lussac's law.

T₁/P₁ = T₂/P₂

T₂ = T₁ × P₂/P₁

T₂ = 280 K × 1.5 atm/3 atm = 140 K

6 0
3 years ago
How many liters of hydrogen are required to react completely with 2.4L of oxygen to form water? 2H2 + O2 --> 2H2O
RoseWind [281]

Answer:

2.4 mole of oxygen will react with 2.4 moles of hydrogen

Explanation:

As we know

1 liter = 1000 grams

2H2 + O2 --> 2H2O

Weight of H2 molecule = 2.016 g/mol

Weight of water = 18.01 gram /l

2 mole of oxygen react with 2 mole of H2

2.4 mole of oxygen will react with 2.4 moles of hydrogen

3 0
2 years ago
If there are 4 grams of product produced by the chemical reaction, how many grams of reactant were consumed?
Colt1911 [192]
D 4 grams
i need to write a couple more character for explanation so there
8 0
3 years ago
Read 2 more answers
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