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3 years ago

What does carbon dioxide do when released into the air

2 answers:

5 0

There are both natural and human sources of carbon dioxide emissions. Natural sources include decomposition, ocean release and respiration. Human sources come from activities like cement production, deforestation as well as the burning of fossil fuels like coal, oil and natural gas.
hopes this helps

Brut [27]3 years ago

3 0

It dissolved into water, then plants uses that carbon create glucose (sugar). Hope this helped

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An object with a mass of 3.2kg has a force of 16.3 newtons to the right and 6.7 newtons to the left applied to it. What is the r

Pepsi [2]

Answer:

3m/s²

Explanation:

Given parameters:

Mass of object = 3.2kg

Force to the right = 16.3N

Force to the left = 6.7N

Unknown:

Acceleration of the object = ?

Solution:

To solve this problem, we use newtons second law of motion;

Net force = mass x acceleration

Net force on object = Force to the right - Force to the left

Net force = 16.3N - 6.7N = 9.6N

So;

9.6 = 3.2 x a

a = $\frac{9.6}{3.2}$ = 3m/s²

7 0

2 years ago

a light ray hits a hard, opaque object. the angle at which the light ray bounces off the object depends on the smoothness of the

kumpel [21]

The answer would be the third option. (the angle at which the light hits the surface.)

8 0

3 years ago

Read 2 more answers

Do liquids have higher coefficients of expansion than solids do

zmey [24]

Answer: yes they do.

Explanation:

I'm tryna get more points because my other account got blocked for the next 48 hours.

(Don't be mad at me please)

4 0

3 years ago

What mass of NaC6H5COO should be added to 1.5 L of 0.40 M C6H5COOH solution at 25 °C to produce a solution with a pH of 3.87 giv

statuscvo [17]

Answer:

41 g

Explanation:

We have a buffer formed by a weak acid (C₆H₅COOH) and its conjugate base (C₆H₅COO⁻ coming from NaC₆H₅COO). We can find the concentration of C₆H₅COO⁻ (and therefore of NaC₆H₅COO) using the Henderson-Hasselbach equation.

pH = pKa + log [C₆H₅COO⁻]/[C₆H₅COOH]

pH - pKa = log [C₆H₅COO⁻] - log [C₆H₅COOH]

log [C₆H₅COO⁻] = pH - pKa + log [C₆H₅COOH]

log [C₆H₅COO⁻] = 3.87 - (-log 6.5 × 10⁻⁵) + log 0.40

[C₆H₅COO⁻] = [NaC₆H₅COO] = 0.19 M

We can find the mass of NaC₆H₅COO using the following expression.

M = mass NaC₆H₅COO / molar mass NaC₆H₅COO × liters of solution

mass NaC₆H₅COO = M × molar mass NaC₆H₅COO × liters of solution

mass NaC₆H₅COO = 0.19 mol/L × 144.1032 g/mol × 1.5 L

mass NaC₆H₅COO = 41 g

7 0

3 years ago

Consider the process used to produce iron metal from its ore.

Dmitry_Shevchenko [17]

Answer:

223.4 grams of iron can be produced from 2.5 moles of Fe2O3 and 6.0 moles of CO.

Explanation:

The balanced reaction is:

Fe₂O₃ (s) + 3 CO(g) → 2 Fe(s) + 3 CO₂ (g)

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of reactant and product participate in the reaction:

Fe₂O₃: 1 mole
CO: 3 moles
Fe: 2 moles
CO₂: 3 moles

Being:

Fe: 55.85 g/mole
O: 16 g/mole
C: 12 g/mole

the molar mass of the compounds participating in the reaction is:

Fe₂O₃: 2*55.85 g/mole + 3*16 g/mole= 159.7 g/mole
CO: 12 g/mole + 16 g/mole= 28 g/mole
Fe: 55.85 g/mole
CO₂: 12 g/mole + 2*16 g/mole= 44 g/mole

Then, by stoichiometry of the reaction, the following quantities participate in the reaction:

Fe₂O₃: 1 mole* 159.7 g/mole= 159.7 g
CO: 3 moles* 28 g/mole= 84 g
Fe: 2 moles* 55.85 g/mole= 111.7 g
CO₂: 3 moles* 44 g/mole= 132 g

The limiting reagent is one that is consumed first in its entirety, determining the amount of product in the reaction. When the limiting reagent is finished, the chemical reaction will stop.

So, first of all, you can apply the following rule of three: if by reaction stoichiometry 1 mole of Fe₂O₃ reacts with 3 moles of CO, then 2.5 moles of Fe₂O₃ react with how many moles of CO?

$moles of CO=\frac{2.5 moles of Fe_{2} O_{3}*3 moles of CO }{1 mole of Fe_{2} O_{3}}$

moles of CO= 7.5

But 7.5 moles of CO are not available, 6.0 moles are available. Since you have less moles than you need to react with 2.5 moles of Fe₂O₃, CO will be the limiting reagent.

Now you can apply the following rule of three: if by reaction stoichiometry 3 moles of CO produce with 111.7 grams of Fe, then 6 moles of CO will produce how much mass of Fe?

$mass of Fe=\frac{6 moles of CO*111.7 grams of Fe}{3 moles of CO}$

mass of Fe= 223.4 grams

223.4 grams of iron can be produced from 2.5 moles of Fe2O3 and 6.0 moles of CO.

5 0

2 years ago