All categories

3 years ago

The circulatory system works with other systems to (select all that apply)

Chemistry

1 answer:

jeka57 [31]3 years ago

7 0

Answer:

where are the answer choices

You might be interested in

H2(g) + F2(g) → 2 HF(g) ΔH=-546 kJ

Arisa [49]

Answer: help please !!

Explanation:

4 0

3 years ago

Read 2 more answers

Staples and metal shavings are examples of which type of hazards

asambeis [7]

They are examples of physical<span> contaminants .</span>

8 0

3 years ago

10. pls pls help me

vagabundo [1.1K]

Answer:

2c2h2+502=4co2+H2O

Explanation:

this is the answer

8 0

3 years ago

Calculate the standard potential for the following galvanic cell: Fe(s) | Fe2+(aq) || Ag+(aq) | Ag(s) which has the overall bala

Nataly [62]

Answer:

E° = 1.24 V

Explanation:

Let's consider the following galvanic cell: Fe(s) | Fe²⁺(aq) || Ag⁺(aq) | Ag(s)

According to this notation, Fe is in the anode (where oxidation occurs) and Ag is in the cathode (where reduction occurs). The corresponding half-reactions are:

Anode: Fe(s) ⇒ Fe²⁺(aq) + 2 e⁻

Cathode: Ag⁺(aq) + 1 e⁻ ⇒ Ag(s)

The standard cell potential (E°) is the difference between the standard reduction potential of the cathode and the standard reduction potential of the anode.

E° = E°red, cat - E°red, an

E° = 0.80 V - (-0.44 V) = 1.24 V

6 0

3 years ago

A 0.187 M weak acid solution has a pH of 3.99. Find Ka for the acid. Express your answer using two significant figures.

Anna35 [415]

Answer:

5.56 × 10⁻⁸

Explanation:

Step 1: Given data

Concentration of the weak acid (Ca): 0.187 M

pH of the solution: 3.99

Step 2: Calculate the concentration of H⁺

We will use the following expression.

pH = -log [H⁺]

[H⁺] = antilog -pH = antilog -3.99 = 1.02 × 10⁻⁴ M

Step 3: Calculate the acid dissociation constant (Ka)

We will use the following expression.

$Ka = \frac{[H^{+}]^{2} }{Ca} = \frac{(1.02 \times 10^{-4})^{2} }{0.187} = 5.56 \times 10^{-8}$

3 0

3 years ago