H2PO4-(aq) ⇆ H+(aq) + HPO42-( which ion plays the role of hydrogen ion donor and which one plays the hydrogen ion acceptor in BP

Answer:

The glycerol solution has a molality of 2.960×10^-2 mol/kg.

Explanation:

Calculating the moles of glycerol involves the formula: Moles = Molarity × Volume of solution = 2.950×10^-2 M × 1 L = 2.950×10^-2 moles.

To find the mass of water, use: Mass = Density × Volume = 0.9982 g/mL × 998.7 mL = 996.90 g, which converts to 0.9969 kg.

The formula for molality is: Molality = Moles of solute/Mass of solvent (in kg) = 2.950×10^-2/0.9969 = 2.960×10^-2 mol/kg.

Response:

CRYSTAL

A LARGE NUMBER OF ATOMS ORGANIZED IN A REGULAR STRUCTURE

1:1

Reasoning:

Answer:

15.71g

Explanation:

The combustion equation that applies to hydrocarbons is

CxHy + (x+y/4) O2 = xCO2 + (y/2) H2O

In the case of octane, C8H18:

C8H18 + ( 8 + 18/4 ) O2 = 8CO2 + 9H2O

C8H18 + 50/4 O2 = 8CO2 + 9H2O

C8H18 + 25/2 O2 = 8CO2 + 9H2O

2C8H18 + 25 O2 = 16 CO2 + 18H2O (this is the balanced equation)

From this balanced reaction,

2 x 22.4 L of octane generates 16 [ 12 + (16 x 2)] of carbon dioxide

That means,

44.8 L of octane generates 704g of carbon dioxide

Thus, for 1L of octane, it produces 1 L x 704g/44.8 L = 15.71g of carbon dioxide

Consequently, 15.71g of carbon dioxide is produced from the complete combustion of 1 L of octane.

Answer:

The heat capacity of the calorimeter is = 54.4

Explanation:

Given the data

Heat supplied Q = 4.168 KJ = 4168 J

Mass of water = 75.40 gm

Change in temperature = ΔT = 35.82 - 24.58 = 11.24 °C

From the conditions provided

Q = ΔT + ΔT

Plugging all values into the above equation yields

4168 = 75.70 × 4.18 × 11.24 +   × 11.24

611.37 =   × 11.24

= 54.4

This represents the heat capacity of the calorimeter.