All categories

3 years ago

How many moles are in 566 grams of CO2? Molar mass of CO2 = 44.0 g/mol

Chemistry

1 answer:

VARVARA [1.3K]3 years ago

5 0

Answer:

Co2 grams to moles

How many grams CO2 in 1 mol? The answer is 44.0095. We assume you are converting between grams CO2 and mole. You can view more details on each measurement unit: molecular weight of CO2 or mol This compound is also known as Carbon Dioxide.

Explanation:

You might be interested in

Can someone help me?

Oduvanchick [21]

Answer:

an element with a large number of valence electrons and a large atomic radius

Explanation:

Electronegativity means a tedency when an atom attracts bonding electrons in a covalent bond situation.

» If an atom has many valency electrons [ empty orbitals in outermost shell ], it has difficulty in attracting electrons hence electronegativity low.

» If an atom is large, its nuclear attraction force of incoming electrons is low hence low electronegativity.

$.$

7 0

3 years ago

What will happen to a salt water fish if placed in freshwater?

Zigmanuir [339]

Answer:

they will die because they need to be in salt water

5 0

3 years ago

Based on Gay-Lussac's law, which of the following statements is true for an ideal gas at constant volume and mole amount? (4 poi

Andreas93 [3]

Is Gay-Lussac really gay?

5 0

3 years ago

A 3.00-L flask is filled with gaseous ammonia, NH3. The gas pressure measured at 27.0 ∘C is 2.55 atm . Assuming ideal gas behavi

Whitepunk [10]

Answer : The mass of ammonia present in the flask in three significant figures are, 5.28 grams.

Solution :

Using ideal gas equation,

$PV=nRT\\\\PV=\frac{w}{M}\times RT$

where,

n = number of moles of gas

w = mass of ammonia gas = ?

P = pressure of the ammonia gas = 2.55 atm

T = temperature of the ammonia gas = $27^oC=273+27=300K$

M = molar mass of ammonia gas = 17 g/mole

R = gas constant = 0.0821 L.atm/mole.K

V = volume of ammonia gas = 3.00 L

Now put all the given values in the above equation, we get the mass of ammonia gas.

$(2.55atm)\times (3.00L)=\frac{w}{17g/mole}\times (0.0821L.atm/mole.K)\times (300K)$

$w=5.28g$

Therefore, the mass of ammonia present in the flask in three significant figures are, 5.28 grams.

8 0

4 years ago

Write the balanced reaction and solubility product expression (KSP) for dissolving silver chromate: Ag2CrO4(s). Include all char

Sonbull [250]

Answer:

2Ag⁺ (aq) + CrO₄⁻² (aq) ⇄ Ag₂CrO₄ (s) ↓

Ksp = [2s]² . [s] → 4s³

Explanation:

Ag₂CrO₄ → 2Ag⁺ + CrO₄⁻²

Chromate silver is a ionic salt that can be dissociated. When we have a mixture of both ions, we can produce the salt which is a precipitated.

2Ag⁺ (aq) + CrO₄⁻² (aq) ⇄ Ag₂CrO₄ (s) ↓ Ksp

That's the expression for the precipitation equilibrium.

To determine the solubility product expression, we work with the Ksp

Ag₂CrO₄ (s) ⇄ 2Ag⁺ (aq) + CrO₄⁻² (aq) Ksp

2 s s

Look the stoichiometry is 1:2, between the salt and the silver.

Ksp = [2s]² . [s] → 4s³

3 0

3 years ago