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3 years ago

Substances made of two or more elements chemically joined togethher are called what

Chemistry

1 answer:

slamgirl [31]3 years ago

7 0

Answer:

compounds

Explanation:

Substances made of two or more elements that are chemically joined together are called <u>compounds</u>.

<em>Generally, elements are substances that contain just a type of atom. Compounds, on the other hand, contain different atoms (of different elements) that are chemically linked together. The linkage is referred to as bonding. The bonding could be covalent, ionic, or hydrogen bonding.</em>

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Cis-platin is a chlorine-containing chemotherapy agent with the formula pt(nh3)2cl2. What is the mass of one mole of cis-platin?

marishachu [46]

Cis-platin is a chemotherapy agent used to treat and kill cancerous cells in patients. One mole of cis-platin has a mass of 300.06 grams/mol. Thus, option B is correct.

<h3>What is a chemotherapy agent?</h3>

A chemotherapy agent is an alkylating agent that is used to treat cancer and is given to reduce the infection or to relieve the symptoms. Cis-platin (Pt(NH₃)₂Cl₂) is one of the chemotherapy agents that treat lung, ovarian, and neck cancer, etc.

The mass of one mole of Cis-platin is calculated as,

Moles = mass ÷ molar mass

Where,

Moles = 1 mole

The molar mass of (Pt(NH₃)₂Cl₂) is calculated as,

195.06 g/mole + 2(17g/mole) + (35.5)2 = 300.06 grams

Substituting values to calculate mass:

Mass = Molar mass × moles

= 300. 06 × 1

= 300.06 grams/mol

Therefore, option B. 300.06 gm/mol is the mass of Cis-platin.

Learn more about chemotherapy agents here:

brainly.com/question/14260402

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Your question is incomplete, but most probably your full question was, Cis-platin is a chlorine-containing chemotherapy agent with the formula pt(nh3)2cl2. What is the mass of one mole of cis-platin?

488.91 g/mol
300.06 g/mol
492.37 g/mol
283.02 g/mol
2860.5 g/mol

8 0

2 years ago

Use the following equation to answer the questions and please show all work.

DIA [1.3K]

Answer:

a.36 g of water is produced.

b.64 g of $O_{2}$ is consumed.

Explanation:

The reaction is $2H_{2} + O_{2}$ ⇒ $2H_{2}O$

Given,

Weight of $H_{2}$ reacted = 4g

Weight of 1 mole of $H_{2}$ = 2 $\times$ 1 = 2g

Therefore no. of moles of $H_{2}$ reacted = $\frac{4}{2}$ = 2 moles;

Also given,

Weight of $O_{2}$ reacted = 32 g

Weight of 1 mole of $O_{2}$ = 2 $\times$ 16 = 32 g

Therefore no. of moles of $O_{2}$ reacted = $\frac{32}{32}$ = 1

We know that 2 moles of Hydrogen reacts with 1 mole of Oxygen to give 2 moles of water,

As we took 2 moles of Hydrogen and 1 mole of Oxygen,

Directly,from the equation we can tell 2moles of water will be produced.

Therefore no. of moles of $H_{2} O$ produced = 2

Weight of 1 mole of water = $2\times 1+16$ = 18

Therefore weight of $H_{2}O$ produced = $2\times 18$ = 36gm

Given ,

72 g of $H_{2}O$ is produced.

So,

no. of moles of $H_{2}O$ produced = $\frac{72}{18}$ = 4 moles

From equation For every 2 moles of water formed , 1 mole of oxygen must be required.

So for producing 4 moles of water,

No. of moles of Oxygen required = 2 moles.

Therefore weight of $O_{2}$ reacted = $2\times32$ = 64 g

Method 2:

Given,

8 g of $H_{2}$ has reacted.

So,

no. of moles of $H_{2}$ reacted = $\frac{8}{2}$ = 4 moles.

From equation , we know that For every 2 moles of $H_{2}$ reacted,1 mole of $O_{2}$ will react.

Therefore,

No. of moles of $O_{2}$ that reacts with 4 moles of $H_{2}$ = $2\times1$ = 2 moles

Therefore the weight of $O_{2}$ reacted = $2\times 32$ = 64 g

6 0

3 years ago

A student must use 220 mL of hot water in a lab procedure. Calculate the amount of heat required to raise the temperature of 220

Inessa [10]

Answer:

64,433.6 Joules

Explanation:

<u>We are given</u>;

Volume of water as 220 mL
Initial temperature as 30°C
Final temperature as 100°C
Specific heat capacity of water as 4.184 J/g°C

We are required to calculate the amount of heat required to raise the temperature.

We know that amount of heat is calculated by;

Q = mcΔT , where m is the mass, c is the specific heat, ΔT is the change in temperature.

Density of water is 1 g/mL

Thus, mass of water is 220 g

ΔT = 100°C - 30°C

= 70°C

Therefore;

Amount of heat, Q = 220g × 4.184 J/g°C × 70°C

= 64,433.6 Joules

Thus, the amount of heat required to raise the temperature of water is 64,433.6 Joules

7 0

3 years ago

An analytical chemist is titrating 242.5 mL of a 1.200 M solution of hydrazoic acid HN3 with a 0.3400 M solution of NaOH. The pK

rodikova [14]

Answer:

The pH of the solution is 12.61

Explanation:

Step 1: Data given

Molarity of hydrazoic acid solution = 1.200 M

Volume of solution = 242.5 mL

Molarity of NaOH solution = 0.3400 M

pKa = 4.72

Step 2: The balanced equation

HN3 + NaOH → NaN3 + H2O

Step 3: Calculate moles hydrazoic acid

Moles hydrazoic acid = molarity * volume

Moles hydra

zoic acid = 1.200 M * 0.2425 L

Moles hydrazoic acid = 0.291 moles

Step 4: Calculate moles NaOH

Moles NaOH = 0.3400 M * 1.006 L

Moles NaOH = 0.342 moles

Step 5: Calculate the limiting reactant

HN3 is the limiting reactant. It will completely be consumed (0.291 moles)

NaOH is in excess. There reacts 0.29 moles. There will remain 0.342 - 0.291 = 0.051 moles NaOH

Step 6: Calculate total volume

Total volume = 242.5 mL + 1006 mL = 1248.5 mL = 1.2485 L

Step 7: Calculate molarity of NaOH

Molarity NaOH = 0.051 moles / 1.2485 L

Molarity NaOH = 0.0408 M

Step 8: Calculate pOH

pOH = -log [OH-] = -log(0.0408)

pOH = 1.39

Step 9: Calculate pH

pH = 14 - pOH

pH = 14 - 1.39

pH = 12.61

The pH of the solution is 12.61

7 0

3 years ago

How many grams of Al2O3 are produced from 4.2 grams of of Al reacting with O2?

butalik [34]

Answer:

1400

Explanation:

3 0

3 years ago