several of the flame tests were shades of red. what should be done in the laboratory to correctly identify one of these ions

A 0.875-g sample of anthracite coal was burned in a bomb calorimeter. The temperature rose from 22.50 to 23.80°C. The heat capac

kherson [118]

Answer:

a) 26.65 kJ was the heat evolved by the reaction.

b) $3.046\times 10^7 kJ$ is the energy released on burning 1 metric ton of this type of coal

Explanation:

Heat capacity of the calorimeter = C = 20.5 kJ/°C

Initial temperature of the calorimeter, $T_1$ = 22.50°C

Final temperature of the calorimeter, $T_2$ = 23.80°C

The heat evolved by the reaction = Q

$Q=C(T_2-T_1)$

$Q=20.5 kJ/^oC\times (23.80^oC-22.50^oC)$

$Q=26.65 kJ$

26.65 kJ was the heat evolved by the reaction.

0.875 g sample of anthracite coal was burned in a bomb calorimeter

0.875 g sample of anthracite coal gives 26.65 kJ of heat.

1 metric ton= 1000 kg

1000 kg = 1000 × 1000 g = 1,000,000 (1 kg =1000 g)

Then burning 1,000,000 g coal will give:

$=\frac{26.65 kJ }{0.875}\times 1,000,000 g=3.046\times 10^7 kJ$

$3.046\times 10^7 kJ$ is the energy released on burning 1 metric ton of this type of coal

8 0

3 years ago

What volume of 0.200 M ethanol solution contains each of the following amounts?

Papessa [141]

Answer:

A. 2.3 L

B. 6.10 L

C. 0.060 L

Explanation:

The question asks the volume of a 0.200 M solution of ethanol that contains certain number of moles of ethanol.

The M in the 0.200 M stands for Molarity. This is a unit of concentration that can be expressed as:

Molarity = moles of solute / Liters of solution

In this case:

0.200 M = moles of ethanol / Liters of solution

So from the formula we can get that we can calculate the volume of the solution, as Liters of solution, given the moles in each case as:

Liters of solution = moles of ethanol / 0.200 moles/L

_______________________________________________

A. 0.45 mol ethanol

Liters of solution = 0.45 moles / 0.200 moles/L = 2.25 L = 2.3 L

B. 1.22 mol ethanol

Liters of solution = 1.22 moles / 0.200 moles/L = 6.10 L

C. 1.2 x 10⁻² mol ethanol

Liters of solution = 1.2 x 10⁻² moles / 0.200 moles/L = 0.060 L

_______________________________________________

Note: Each answer is given with the correct number of significant figures which results from the least number of significant figures in the given used values in each calculation.

7 0

3 years ago

Two technicians are discussing ASE certification. Technician A says that there are 60-plus exams each designed to discern the au

finlep [7]

Answer:

Technician B is correct.

Explanation:

ASE exams are in 9 categories and they're based on real things that would happen in service shops in real life.

4 0

3 years ago

A storm that stays longer over coasts is a more dangerous storm. Is this statement true or false?

11Alexandr11 [23.1K]

Answer:

I think it is true, but I am not to sure.

5 0

3 years ago

Read 2 more answers

The mass percentage of hydrochloric acid within a solution is 15.00%. given that the density of this solution is 1.075 g/ml, fin

Morgarella [4.7K]

Given the mass percentage of HCl solution = 15.00 %

This means that 15.00 g HCl is present in 100 g solution

Moles of HCl = $15.00 gHCl*\frac{1 mol HCl}{36.46 g HCl} =0.411molHCl$

Density of the solution = 1.075 g/mL

Calculating the volume of solution from density and mass:

$100 g *\frac{1mL}{1.075 g} =93.0 mL$

Converting volume from mL to L:

$93.0 mL * \frac{1 L}{1000 mL} =0.093 L$

Calculating the molarity of HCl solution from moles and volume:

$\frac{0.411 mol}{0.093 L} =4.42 mol/L$

8 0

4 years ago