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3 years ago

60 points please help me i will appreciate it!

Chemistry

1 answer:

Setler79 [48]3 years ago

4 0

Answer:

$\huge\boxed{\sf T = 682.4 \ K}$

Explanation:

Given Data:

Mole = n = 0.1 mol

Pressure = P = 530 mmHg = 0.7 atm

Volume = v = 8 L

Ideal gas constant = R = 0.8206 L atm K⁻¹ mol⁻¹

Required:

Temperature = T = ?

Formula:

Pv = nRT

Solution:

Rearranging for T

$\displaystyle T = \frac{Pv}{nR} \\\\T = \frac{(0.7)(8)}{(0.1)(0.08206)} \\\\T = \frac{5.6}{0.008206} \\\\T = 682.4 \ K\\\\\rule[225]{225}{2}$

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When heated, magnesium combines readily with excess oxygen in the air to produce magnesium oxide, as shown in the following unba

aev [14]

Answer: The given chemical reaction can be classified as synthesis and exothermic.

Explanation:

A synthesis reaction is defined as the reaction where two small chemical species combine in their elemental state to form a single large chemical species.

Exothermic reactions are defined as the reactions in which heat is released by the reaction. The heat is written on the product side of the reaction.

For the given chemical reaction:

$Mg(s)+O_2(g)\rightarrow MgO(s)+\text{heat}$

The above chemical reaction is a type of synthesis and exothermic as two substances in their elemental state are combining. Also, heat is getting released in the reaction.

Hence, the given chemical reaction can be classified as synthesis and exothermic.

4 0

3 years ago

Help asap!!!!!!!!!!!

ivann1987 [24]

Your answer to #2 is There are several differences between a physical and chemical change in matter or substances. A physical change in a substance doesn't change what the substance is. In a chemical change where there is a chemical reaction, a new substance is formed and energy is either given off or absorbed.

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3 years ago

The standard free energy of activation of one reaction A is 95.00 kJ mol–1 (22.71 kcal mol–1). The standard free energy of activ

diamong [38]

Answer:

The answer to the questions are as follows

Reaction B is 4426.28 times faster than reaction A

(b) Reaction B is faster.

Explanation:

To solve the question we are meant to compare both reactions to see which one is faster

The values of the given activation energies are as follows

For A

Ea = 95.00 kJ mol–1 (22.71 kcal mol–1) and

for B

Ea = 74.20 kJ mol–1 (17.73 kcal mol–1)

T is the same for both reactions and is equal to 298 k

Concentration of both reaction = 1M

The Arrhenius Law is given by

k = $Ae^{\frac{-E_{a} }{RT} }$

Where

k = rate constant

Ea = activation energy

R = universal gas constant

T = temperature (Kelvin )

A = Arrhenius factor

Therefore

For reaction A, the rate constant k₁ is given by k₁ = $Ae^{\frac{-95000}{(8.314)(298)} }$

And for B the rate constant k₂ is given by k₂ = $Ae^{\frac{-74200 }{(8.314)(298)} }$

k₁ = A×2.225×10⁻¹⁷

k₂ = A×9.850×10⁻¹⁴

As seen from the above Reaction B is faster than reaction A by (A×9.850×10⁻¹⁴)/(A×2.225×10⁻¹⁷) or 4426.28 times

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3 years ago

The exhaust gas from an automobile contains 1.5 percent by volume of carbon monoxide. What is the concentration of CO in mg/m' a

FrozenT [24]

Answer:

(a) 17,178 mg/m3

(b) 11,625 mg/m3

Explanation:

The concentration of CO in mg/m3 can be calculated as

$C (mg/m3) =(P/RT)*MW*C_{ppm}$

For standard conditions (1 atm and 25°C), P/RT is 0.0409.

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$C=(P/RT)*MW*C_{ppm}\\\\C=0.0409*28*15,000=17,178$

(b) For 200°C and 1.1 atm,

$P/RT=0.0409*(P/P_{std})*(T_{std}/T)\\P/RT=0.0409*(1.1atm/1atm)*(273+15K/273+200K)=0.0277$

Then the concentration in mg/m3 is

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5 0

3 years ago

Competition occurs when

Katen [24]

Answer:

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Explanation:

I dont think it could be (B), (C) or (D) because those don't really make sense.

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2 years ago