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2 years ago

3) (4.5 x 10-14) x (5.2 x 103) = ?

Chemistry

2 answers:

snow_tiger [21]2 years ago

5 0

Answer:

16,603.6

Explanation:

(4.5 x 10 - 14) x (5.2 x 103)

(45 -14) x 535.6

31 x 535.6

16,603.6

Otrada [13]2 years ago

4 0

Answer:

16603.6

1.66036 x 10^4

Hope this helps! ^_^

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How can scientists control the flammability of a substance?

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Answer: This is simple, if it has a high flammability, and you light it on fire, then that would be a chemical change.

Explanation:

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2 years ago

A reaction between substances Y and Z is

Anuta_ua [19.1K]

Answer : The value of activation energy for this reaction is 108.318 kJ/mol

Explanation :

The Arrhenius equation is written as:

$K=A\times e^{\frac{-Ea}{RT}}$

Taking logarithm on both the sides, we get:

$\ln k=-\frac{Ea}{RT}+\ln A$ ............(1)

where,

k = rate constant = $2.95\times 10^{-3}L/mol.s$

Ea = activation energy = ?

T = temperature = 435 K

R = gas constant = 8.314 J/K.mole

A = pre-exponential factor = $3.00\times 10^{+10}L/mol.s$

Now we have to calculate the value of rate constant by putting the given values in equation 1, we get:

$\ln (2.95\times 10^{-3}L/mol.s)=-\frac{Ea}{8.314J/K.mol\times 435K}+\ln (3.00\times 10^{10}L/mol.s)$

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2 years ago

24g of methane were burned in an excess of air. What mass of water would be produced in the reaction assuming complete combustio

expeople1 [14]

Answer:

54g of water

Explanation:

Based on the reaction, 1 mole of methane produce 2 moles of water.

To solve this question we must find the molar mass of methane in order to find the moles of methane added. With the moles of methane and the chemical equation we can find the moles of water produced and its mass:

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1C = 12g/mol*1

4H = 1g/mol*4

12g/mol + 4g/mol = 16g/mol

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Moles water:

1.5moles CH₄ * (2mol H₂O / 1mol CH₄) = 3.0moles H₂O

Molar mass water:

2H = 1g/mol*2

1O = 16g/mol*1

2g/mol + 16g/mol = 18g/mol

Mass water:

3.0moles H₂O * (18g / mol) =

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3 years ago

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