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sashaice [31]
3 years ago
9

What is the percent by mass of oxygen in carbon dioxide (CO2)?

Chemistry
1 answer:
wariber [46]3 years ago
8 0

Answer:

= 72.73%

Explanation:

The percentage by mass of an element is given by;

% element = total mass of element in compounds/molar mass of compound × 100

The mass of oxygen in carbon dioxide = 32 g

Molar mass of CO2 = 44 g

Therefore;

% of O2 = 32/44 × 100%

             <u>= 72.73%</u>

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What type of forces allow for an object to stay at rest or continue at constant velocity.
galina1969 [7]

Answer:Inertia is the property of a body to remain at rest or to remain in motion with constant velocity. Some objects have more inertia than others because the inertia of an object is equivalent to its mass.

Explanation:

5 0
3 years ago
Read 2 more answers
When salt is placed on ice the ice melts explain why?​
jekas [21]

Answer: The addition of salt in ice particles causes a decrease on its freezing point.

Explanation: salt definitely lowers the freezing point of ice particles.

5 0
3 years ago
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What is the threshold frequency ν0 of cesium?
Montano1993 [528]
 I think this is what you're after:

 Cs(g) → Cs^+ + e⁻ ΔHIP = 375.7 kJ mol^-1 [1] 


Convert to J and divide by the Avogadro Const to give E in J per photon 


E = 375700/6.022×10^23 = 6.239×10^-19 J 


Plank relationship E = h×ν E in J ν = frequency (Hz s-1) 


Planck constant h = 6.626×10^-34 J s 


6.239×10^-19 = (6.626×10^-34)ν 


ν = 9.42×10^14 s^-1 (Hz) 


IP are usually given in ev Cs 3.894 eV 


<span>E = 3.894×1.60×10^-19 = 6.230×10^-19 J per photon </span>

4 0
3 years ago
The density of H2O2 is 1.407 g/mL, and the density of O2 is 1.428 g/L. How many liters of O2 can be made from 55 mL H2O2
balandron [24]

Explanation:

mass H2O2 = 55 mL(1.407 g/mL) = 80.85 g

molar mass H2O2 = 2(1.01 g/mol) + 2(16.00 g/mol) = 34.02 g/mol

moles H2O2 = 80.85 g/34.02 g/mol = 2.377 moles H2O2

For each mole of H2O2 you obtain 0.5 mole of O2 (see the equation).

moles O2 = 2.377 moles H2O2 (1 mole O2)/(2 moles H2O2) = 1.188 moles O2

Now, you need the temperature.  If you are at STP (273 K, and 1.00 atm) then 1 mole of an ideal gas at STP has a volume of 22.4 L.  Without temperature you are not really able to continue.  I will assume you are at STP.

Volume O2 = 1.188 moles O2(22.4 L/mole) = 0.0530 L of O2.

which is  53 mL.

8 0
2 years ago
Calculate the work done when an ideal gas expands isothermally and reversibly in a piston and cylinder assembly for expansion of
pantera1 [17]

Answer:

W=5743.1077\ J

Explanation:

The expression for the work done is:

W=RT \ln \left( \dfrac{P_1}{P_2} \right)

Where,

W is the amount of work done by the gas

R is Gas constant having value = 8.314 J / K mol

T is the temperature

P₁ is the initial pressure

P₂ is the final pressure

Given that:

T = 300 K

P₁ = 10 bar

P₂ = 1 bar

Applying in the equation as:

W=8.314\times 300 \ln \left( \dfrac{10}{1} \right)

W=300\times \:8.314\ln \left(10\right)

W=2.30258\times \:2494.2

W=5743.1077\ J

5 0
3 years ago
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