2

Consider the followong balanced reaction. What mads in g of co2 can be formed from 288 mg of o2. Assume that there is excess c3h

Gwar [14]

<u>Answer:</u>

<em>0.264 g of $CO_2$ can be formed from 288 mg of $O_2$ </em>

<u>Explanation:</u>

The balanced chemical equation is

$2 C_3 H_7 OH+9 O_2> 6 CO_2+8 H_2 O$

The conversions are

Mass in mg $O_2$ is converted to mass in g $O_2$

Mass in g $O_2$ is converted to moles $O_2$ by dividing with molar mass

Moles $O_2$ is converted to moles $CO_2$ by using the mole ratio of $O_2:CO_2$ is 9 : 6

Moles $CO_2$ is converted to mass $CO_2$ by multiplying with molar mass $CO_2$

mass in mg $O_2$ > mass in g $O_2$ >moles $O_2$ > moles $CO_2$ > mass $CO_2$

$288mg O_2 \times \frac{(1g O_2)}{(1000mg O_2 )} \times \frac {(1molO_2)}{(32gO_2 )}\times\frac {(6mol CO_2)}{(9mol O_2 )} \times \frac {(44.0 gCO_2)}{(1mol CO_2 )}$

=0.264g (Answer)

7 0

3 years ago

The two systems that control your body functions are the

KatRina [158]

c) nervous and endocrine system

Hope I helped! ( Smiles )

5 0

2 years ago

Adding 5.25 g of to 130 g of water in a coffee-cup calorimeter (with stirring to dissolve the salt) resulted in a decrease in te

xxTIMURxx [149]

Answer:

ΔHrxn = - 1534.3 J

Explanation:

Given the assumptions and the formula for the change in enthalpy:

ΔHrxn = m x C x ΔT, where

m is the mass of solution given 135.4 g

C is the heat capacity 4.2 J/g .K and,

ΔT is the change in temperature

we have ,

T₁ = ( 18.1 + 273) K = 291.1 K

T₂ = ( 15.4 +273) K = 288.4 K

ΔHrxn = 135.3 g x 4.2 J/gK x ( 288.4 -291.1 ) K = - 1534.3 J

After verifying our result has the correct unit, the answer is -1534.3 Joules, and the negative sign tells us it is an endothermic reaction decreasing the final temperature.

4 0

2 years ago

what type of orbital is occupied by an electron with the quantum numbers n=3, 1=2? How many degenerate orbital's of this type ar

ki77a [65]

Tryna boost my score for college chemistry could you give me the brainiest and a thanks? Hope you find your answer your looking for!

4 0

3 years ago

Determine the pressure in atm exerted by 1 mole of methane placed into a bulb with a volume of 244.6 mL at 25°C. Carry out two c

Nuetrik [128]

The pressure in atm exerted by 1 mole of methane placed into a bulb with a volume of 244.6 mL at 25°C is 101.94atm.

<h3>How to calculate pressure?</h3>

The pressure of an ideal gas can be calculated using the following formula:

PV = nRT

Where;

P = pressure
V = volume
n = number of moles
R = gas law constant
T = temperature

According to information in this question;

T = 25°C = 25 + 273 = 298K
V = 244.6mL = 0.24L
R = 0.0821 Latm/Kmol

P × 0.24 = 1 × 0.0821 × 298

0.24P = 24.47

P = 24.47/0.24

P = 101.94atm

Therefore, the pressure in atm exerted by 1 mole of methane placed into a bulb with a volume of 244.6 mL at 25°C is 101.94atm.

Learn more about pressure at: brainly.com/question/11464844

3 0

2 years ago