Find the amount of heat (Q) needed to raise the temperature of 5.00 g of a substance from 20.0 C to 30.0C if

Why do we have to add acid to water but not water to acid

KATRIN_1 [288]

It should be CAT!!!!

5 0

3 years ago

Please help me with this one

MrRa [10]

Answer: D-Nonmetals bond together to form a covalent compound

6 0

3 years ago

Acid deposition results from burning fossil fuels that release ___________ that react in the atmosphere to form acids that fall

AysviL [449]

Sulfur dioxide. this is the cause

4 0

3 years ago

Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S 2 ( g ) + C ( s ) − ⇀ ↽ − CS 2 ( g ) K c

bezimeni [28]

Answer:

974.6 grams of CS2 can be prepared.

Explanation:

Step 1: Data given

Kc = 9.40 at 900 K

Moles of S2 = 14.2 mol

volume = 6.30 L

Molar mass of CS2 = 76.14 g/mol

Step 2: The balanced equation:

S2(g)+C(s) ↔ CS2(g)

Step 3: Calculate initial concentrations

Concentration of S2 = moles S2 / volume

Concentration of S2 = 14.2 moles / 6.30 L

Concentration of S2 = 2.25 M (This is the initial concentration)

The initial concentration of C and CS2 is 0M

Since the mole ratio is 1:1:1

There will react X

The concentration of S2 at the equilibrium is: (2.25 -X)M

The concentration of C and CS2 at the equilibrium is X M

Step 4: Calculate concentrations

Since C is not a gas but solid, it doesn't matter for the Kc

Kc = 9.40 = (products)/(reactants) = [CS2(g)]/[S2(g)]

9.40 = X/(2.25-X)

X = 2.034 = [CS2]

[S2] = 2.25 - 2.034 = 0.216

Step 5: Calculate moles of CS2

Moles CS2 = molarity CS2 * volume

Moles CS2 = 2.034 M * 6.30 L

Moles CS2 = 12.8 moles

Step 6: Calculate mass of CS2

Mass CS2 = moles CS2 * molar mass CS2

Mass CS2 = 12.8 moles * 76.14 g/mol

Mass CS2 = 974.6 grams

974.6 grams of CS2 can be prepared.

6 0

3 years ago

Express the equilibrium constant for the following reaction.P4O10(s) ↔ P4(s) + 5 O2(g)K = [P4][O2]^5/[P4O10]K = [O2]^5K = [P4O10

Alex17521 [72]

Answer : The correct expression for equilibrium constant will be, $K=[O_2]^5$

Explanation :

Equilibrium constant : It is defined as the equilibrium constant. It is defined as the ratio of concentration of products to the concentration of reactants.

The equilibrium expression for the reaction is determined by multiplying the concentrations of products and divided by the concentrations of the reactants and each concentration is raised to the power that is equal to the coefficient in the balanced reaction.

As we know that the concentrations of pure solids are constant that is they do not change. Thus, they are not included in the equilibrium expression.

The given equilibrium reaction is,

$P_4O_{10}(s)\rightleftharpoons P_4(s)+5O_2(g)$

The expression of $K$ will be,

$K=[O_2]^5$

Therefore, the correct expression for equilibrium constant will be, $K=[O_2]^5$

7 0

3 years ago