All categories

2 years ago

Help please science (7th grade)

Chemistry

2 answers:

hoa [83]2 years ago

8 0

Answer:

Explanation:

Don't mind the random letters

bshsujsjjdjd

tiny-mole [99]2 years ago

8 0

Answer:

Explanation:

You might be interested in

What is 1 +1 (a) 11 (b) 3 (c) 6 (d) 2

Doss [256]

I believe the answer is D) 2

8 0

3 years ago

Read 2 more answers

A 50.0 mL sample of a 1.00 M solution of CuSO4 is mixed with 50.0 mL of 2.00 M KOH in a calorimeter. The temperature of both sol

Reika [66]

Answer : The enthalpy change for the process is 52.5 kJ/mole.

Explanation :

Heat released by the reaction = Heat absorbed by the calorimeter + Heat absorbed by the solution

$q=[q_1+q_2]$

$q=[c_1\times \Delta T+m_2\times c_2\times \Delta T]$

where,

q = heat released by the reaction

$q_1$ = heat absorbed by the calorimeter

$q_2$ = heat absorbed by the solution

$c_1$ = specific heat of calorimeter = $12.1J/^oC$

$c_2$ = specific heat of water = $4.18J/g^oC$

$m_2$ = mass of water or solution = $Density\times Volume=1/mL\times 100.0mL=100.0g$

$\Delta T$ = change in temperature = $T_2-T_1=(26.3-20.2)^oC=6.1^oC$

Now put all the given values in the above formula, we get:

$q=[(12.1J/^oC\times 6.1^oC)+(100.0g\times 4.18J/g^oC\times 6.1^oC)]$

$q=2623.61J$

Now we have to calculate the enthalpy change for the process.

$\Delta H=\frac{q}{n}$

where,

$\Delta H$ = enthalpy change = ?

q = heat released = 2626.61 J

n = number of moles of copper sulfate used = $Concentration\times Volume=1M\times 0.050L=0.050mole$

$\Delta H=\frac{2623.61J}{0.050mole}=52472.2J/mole=52.5kJ/mole$

Therefore, the enthalpy change for the process is 52.5 kJ/mole.

8 0

3 years ago

Gold alloys are _____.

chubhunter [2.5K]

Gold alloys consist of most commonly Nickel!
Most commonly used in things like jewelry so it doesn't have such a heavy weight.

7 0

2 years ago

Can someone please help me and ill mark you as brainlest

r-ruslan [8.4K]

Answer:

can you show the question so we can read it

3 0

3 years ago

Read 2 more answers

The forensic technician at a crime scene has just prepared a luminol stock solution by adding 16.0 g of luminol into a total vol

nikitadnepr [17]

The molarity of the stock solution of luminol is 1.2 M

<u><em>calculation</em></u>

step 1: find the moles of luminol using (moles= mass/molar mass) formula

molar mass of Luminol= 177 g/mol

moles is therefore= 16.0 g/ 177 g/mol=0.0904 moles

Step 2: find the molarity using (molarity= moles/volume in liters) formula

convert Ml into liters = 75.0/1000= 0.075 L

molarity is therefore= 0.0904 moles/ 0.075 L= 1.2M

6 0

3 years ago