Why are many scientists concerned about humans adding large amounts of carbon to the atmosphere by burning fossil fuels (combustion)

Answer:

Explanation:

a) Hydronium ion (H₃O⁺) is the acidic ion, after reacting with a base Calcium hydroxide the pH decreased. The base contained a hydroxide ion (OH⁻) which reacted with the Hydronium ion causing the decrease of hydronium ion.

b) The base which is Calcium hydroxide is made up of Calcium ion (Ca²⁺) and hydroxide ion (OH⁻) which reacts to form Calcium hydroxide [Ca(OH)₂]

Ca²⁺    +       OH⁻     ⇒    Ca(OH)₂

a. The reason of ion that resulted into the decrease of the hydronium ion should be explained below.

b. The formula is Ca²⁺    +       OH⁻     ⇒    Ca(OH)₂.

a) Hydronium ion (H₃O⁺) represent the acidic ion that should be reacted along with the base i.e.  Calcium hydroxide when there should be decrease in the pH. Here the base should comprise of the hydroxide ion (OH⁻) that should be reacted with the Hydronium ion.

b. The formula should be

we know that

The base should be based on Calcium hydroxide comprise of Calcium ion (Ca²⁺) and hydroxide ion (OH⁻)

So, it should be like

Ca²⁺    +       OH⁻     ⇒    Ca(OH)₂

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Answer:

C: C3CI9

Explanation:

Binary Molecular compound states that the molecular formula for tricarbon nonacholride is C3CI9

Hope this helps

Answer:

C

Explanation:

Think about the prefixes to solve this. I've attached a Latin prefix chart. It might help to memorize this!

Tri- carbon means 3 carbons.

Nona- chloride means 9 chlorines.

So the answer is C₃Cl₉.

The reason we use these prefixes is because it's a covalent compound. If it's ionic, we don't need to use the tri- or nona- parts of it.

Answer:

32.4 grams of K3N will be produced

Explanation:

Step 1: Data given

Mass of potassium = 29.0 grams

Mass of barium nitride = 66.5 grams

Atomic mass of potassium = 39.10 g/mol

Molar mass of barium nitride = 440 g/mol

Step 2: The balanced equation

6K + Ba3N2 → 2K3N + 3Ba

Step 3: Calculate moles

Moles = mass / molar mass

Moles K = 29.0 grams / 39.10 g/mol

Moles K = 0.742 moles

Moles Ba3N2 = 66.5 grams / 440 g/mol

Moles Ba3N2 = 0.151 moles

Step 4: Calculate the limiting reactant

For 6 moles K we need 1 mol Ba3N2 to produce 2 moles K3N and 3 moles Ba

K is the limiting reactant. It will completely be consumed (0.742 moles). Ba3N2 is in excess. There will react 0.742/ 6 = 0.124 moles

There will remain 0.151 - 0.124 = 0.027 moles

Step 5: Calculate moles K3N

For 6 moles K we need 1 mol Ba3N2 to produce 2 moles K3N and 3 moles Ba

For 0.742 moles K we'll have 0.742/3 = 0.247 moles K3N

Step 6: Calculate mass K3N

Mass K3N = moles K3N * molar mass K3N

Mass K3N = 0.247 moles * 131.3 g/mol

Mass K3N = 32.4 grams

32.4 grams of K3N will be produced

The question contains a chemical inconsistency regarding potassium nitride. Instead, we reviewed typical precipitation and double displacement reactions where the mass of products and excess reactants are calculated using the principle of limiting reactants and stoichiometry.

The question asks for the mass of potassium nitride produced when potassium reacts with barium nitride. However, this appears to be an error because potassium nitride is not a common compound, and the reaction given is not between potassium and barium nitride. Instead, we can examine a more typical reaction based on the provided examples, which involve precipitation and double displacement reactions.

For the reaction Pb(NO3)2 (aq) + 2 KI (aq) → PbI2 (s) + 2 KNO3 (aq), the limiting reactant principle is applied, whereby the reactant that produces the least amount of product is the limiting reactant. To calculate this, one would first determine the number of moles of each reactant using their respective molar masses, then apply the stoichiometric ratios from the balanced equation.

Similarly, to find out the excess reactant and the mass of products in other reactions such as the reaction between KOH and HNO3, you would apply the same principles to arrive at the desired masses.

Answer:

70g

Explanation:

2*40 of cawill require 112g of cao

50g of ca will require

Ans=70g of cao

The concentration of H3O+ in rainwater with a pH of 4.35 is approximately 3.548 x 10^(-5) M.

The concentration of H3O+ in rainwater with a pH of 4.35 can be calculated using the equation pH = -log[H3O+]. Rearranging the equation to solve for [H3O+], we have [H3O+] = 10^(-pH). Substituting the given pH value into the equation, we find that the [H3O+] concentration is approximately 3.548 x 10^(-5) M.

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Answer:

1.66 atm

Explanation:

P1V1/T1 = P2V2/T2

1.00atm*30.0mL/273K= P2*20.0 mL/303K

P2 = (1.00*30.0*303)/(273*20.0) = 1.66 atm

Answer:

-112°C

Explanation:

Given,

Pressure, P = 971 mmHg

moles of carbon dioxide = 3.3

Temperature, T = ?

Volume = 34.13 L

Pressure in atm = [tex]\dfrac{971}{760} = 1.278\ atm[/tex]

Now, using ideal gas equation

PV = n RT

1.278 x 34.13 =3.3 x 0.08206 x T

T = 161.07 K

Temperature in °C = 161.07-273 = -112°C

Temperature of sample is  -112°C.