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Ray Of Light [21]
3 years ago
7

If 9.5 × 10²⁵ molecules of CO₂ are produced in a combustion reaction, what is the mass in kg of CO₂ that is produced?

Chemistry
1 answer:
Leno4ka [110]3 years ago
4 0

Answer:

6.9428 kg of CO2

Explanation:

1) Use Avogadro's number that states 1 mole = 6.022 x 10^23 particles. Convert 9.5 x 10^25 molecules into moles.

9.5 x 10^25 CO2 moleculesx\frac{1 mole CO2}{6.022 x 10^23} = 157.75 moles CO2

2) Convert 157.75 moles of CO2 into grams. CO2's molar mass is 44.01g.

157.75moles CO2 x \frac{44.01g/mol}{1 mole CO2} = 6942.79g

3) Convert 6942.79 grams into kilograms (divide by 1000):

6.9428 kg

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Viruses are not classified as being alive in because of the fact that they can't reproduce.
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3 years ago
If the human body were a car, glucose would be:
NeTakaya
<span>If the human body were a car, glucose would be the gasoline.
Glucose gives humans energy, we basically run on glucose, among other things, the same way a car would run on gas. 
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8 0
3 years ago
Aqueous sodium phosphate and aqueous iron (III) chloride react to produce aqueous sodium chloride and solid iron (III) phosphate
mojhsa [17]

Answer:

this one is hard

Explanation:

but it's iron because the sodium so yea there u go.

4 0
2 years ago
Titanium and chlorine react to form titanium(IV) chloride, like this:
leva [86]

Answer:

the value of equilibrium constant for the reaction is 8.5 * 10⁷

Explanation:

Ti(s) + 2 Cl₂(g) ⇄ TiCl₄(l)

equilibrium constant Kc = \frac{1}{[Cl_2]^2}

Given that,

We are given:

Equilibrium amount of titanium = 2.93 g

Equilibrium amount of titanium tetrachloride = 2.02 g

Equilibrium amount of chlorine gas = 1.67 g

We calculate the No of mole = mass / molar mass

mass of chlorine gas = 1.67 g

Molar mass of chlorine gas = 71 g/mol

mole of chlorine = 1.67 / 71

= 7.0L

Concentration of chlorine is = no of mole / volume

= 0.024 / 7

= 3.43 * 10⁻³M

equilibrium constant Kc  = \frac{1}{[Cl_2]^2}

= \frac{1}{[3.43 * 10^-^3]^2}

= 8.5 * 10⁷

4 0
3 years ago
How many grams of water vapor (H2O) are in a 10.2 liter sample at 0.98 atmospheres and 26ÁC? Show all work used to solve this pr
klio [65]
The answer is 7.33 g.

<span>To calculate this, we will use the the ideal gas law:
PV = nRT
where
P - pressure of the gas,
V - volume of the gas,
n - amount of substance of gas,
R - gas constant,
T - temperature of the gas.</span>

Since the amount of substance of gas (n) can be expressed as mass (m) divided by molar mass (M), then:

PV = RTm/M

It is given:

P = 0.98 atm

V = 10.2 l

T = 26°C = 299.15 K 

R = 0.082 l atm/Kmol (gas constant)

M (H2O) = 2Ar(H) + Ar(O) = 2*1 + 16 = 2 + 16 = 18g

m = ?

Since PV = RTm/M, then:

m = PVM/RT

m = 0.98 · 10.2 · 18 / 0.082 · 299.15 = 179.928/24.5303 = 7.33 g

6 0
3 years ago
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